2. For the following two compounds between oxygen and hydrogen: 3. Tell what discoveries were made by each of the following scientists:

Size: px
Start display at page:

Download "2. For the following two compounds between oxygen and hydrogen: 3. Tell what discoveries were made by each of the following scientists:"

Transcription

1 EXTRA HOMEWORK 1A 1. When Dalton proposed that matter was composed of atoms, why was his Atomic Theory accepted? 2. For the following two compounds between oxygen and hydrogen: Mass of O Mass of H Compound A 16 grams 1 grams Compound B 16 grams 2 grams (a) Propose formulas for the two compounds assuming that each oxygen atom weighs the same as each hydrogen atom (b) Propose formulas for the two compounds assuming that each oxygen atom weighs 8 times more than each hydrogen atom (c) Propose formulas for the three compounds assuming that each oxygen atom weighs 16 times more than each hydrogen atom 3. Tell what discoveries were made by each of the following scientists: (a) J.J. Thomson (b) Lord Rutherford 4. If a model of a hydrogen atom had a diameter of 45 cm, what would have to be the diameter of the nucleus? *5. Nitrogen forms two compounds with oxygen, and their elemental proportions by mass are: Mass of N Mass of O Compound 1 14 grams 8 grams Compound 2 14 grams 16 grams Compound 3 14 grams 32 grams Assuming the atomic mass of oxygen is 16, predict the simplest formulas of these compounds assuming that (a) Nitrogen has an atomic mass of 14 (b) Nitrogen has an atomic mass of 7 (c) Nitrogen has an atomic mass of 9 1 / 3 *6. Using the masses of a proton and an electron, and the sizes of the atom and the nucleus, determine the denisity of (a) a 1 H atom (b) a 1 H nucleus

2 EXTRA HOMEWORK 1B 1. One of the primary visible emissions from helium occurs at nm. For this given wavelength of light, calculate: (a) the wavelength in meters (b) the frequency (c) the energy of a single photon in joules (d) the energy of 1 mole of photons in kilojoules 2. The energy of electromagnetic radiation needed to remove electrons from the surface of cesium atoms is 231 kj/mol. Calculate: (a) the energy of a single photon of this electromagnetic radiation in joules (b) the frequency of this electromagnetic radiation (c) the wavelength of this electromagnetic radiation, in meters (d) the wavelength of this electromagnetic radiation, in nanometers (e) identify this electromagnetic radiation as either visible light, infrared radiation, or unltraviolet radiation *3. Give the experimental evidence that supports the fact that light behaves as a wave phenomenom when traveling throught space. *4. The work function of an element is the energy required to remove an electron from the surface of the solid element. The work function for lithium is kj/mol (that is, it takes kj of energy to remove one mole of electrons from one mole of lithium atoms on the surface of lithium metal). What is the maximum wave of light that can remove an electron from an atom on the surface of lithium metal? EXTRA HOMEWORK 1C 1. What does it mean if something is quantized? 2. Draw an electronic energy diagram for a hydrogen atom, and using vertical lines show the following 3 transitions: (a) n = 5 n = 2 (b) n = 4 n = 1 (c) n = 2 n = 4 3. Calculate the de Broglie wavelength of an electron moving at 99% the speed of light. 4. What are the results of passing a beam of electrons through two slits? *5. From the Heisenberg uncertainty principle, calculate the uncertainty in position ( x) of a baseball (mass = kg) with v = m/s. (Planck s constant, h, is kgm 2 /s)

3 EXTRA HOMEWORK 1D 1. Tell whether each of the following orbital designations are allowed of forbidden based upon the Schrödinger Equation. (a) 1p (b) 3f (c) 7d (d) 6h 2. Draw a picture of each of the following orbitals. (a) 2s (b) 2p (c) 3p (d) 3d 3. Concerning the fourth energy level of a hydrogen atom, tell: (a) tell the names of each sublevel it has (b) sketch the radial probability distribution for the orbitals of each sublevel 4. Tell what each of the following designations mean. (a) n = 3 (b) n = 8 (c) 4f (d) 2s (e) 7p x (f) 5f yz 2 5. Give the maximum number of electrons in an atom that can have the following designations. (a) n = 4 (b) n = 10 (c) 6d (d) 12s (e) 5py (f) 4d xz (g) 4d z 2 6. Give the orbital notation for the following atoms: (a) C (b) O (c) P *7. Although no currently known elements contain electrons in g orbitals in the ground state, electrons in excited states can be in g orbitals. (a) give the lowest value for n for which a g sublevel exists (b) give the number of electrons that a g sublevel could hold *8. Concerning the sixth energy level of a hydrogen atom, tell: (a) tell the names of each sublevel it has (b) tell the number of orbitals the sixth energy level has

4 EXTRA HOMEWORK 1E 1. Give the electron configuration notations and the electron dot notations for the following atoms: (a) Si (b) Cr (c) Po (d) Pu 2. For the silicon atom from question 1, name and draw pictures of its occupied valence atomic orbitals. 3. Using radial probability distribution graphs, explain why the 4s sublevel fills before the 3d sublevel in the d-block elements. 4. For the following electron configuration notations of sodium, identify each as a ground state electron configuration, an excited state electron configuration, or an impossible electron configuration: (a) 1s 2 2s 2 2p 5 3s 2 (b) 1s 2 2s 2 2p 6 3d 1 (c) 1s 2 2s 2 2p 6 3s 1 (d) 1s 2 2s 2 2p 6 2d 1 5. Using the periodic table, give the number of protons, neutrons and electrons in each of the following atoms: (a) 40 Ca (b) 51 V (c) 79 Br - (d) 252 Cf 6. What is probably the most abundant isotope of thorium? *7. Why does the 2s orbital fill before the 2p orbitals in multielectron atoms? *8. Why does the 4s orbital fill before the 3d orbitals in multielectron atoms? *9. In the ground state of mercury, (a) How many electrons occupy atomic orbitals with n = 3? (b) How many electrons occupy d atomic orbitals? (c) How many electrons occupy p z atomic orbitals? (d) How many electrons have spin up? *10. Which of elements 1-36 (a) have one unpaired electron in its ground state? (b) have two unpaired ectrons in its ground state? *11. Give the electron configuration notations for the following atoms: (a) Mo (b) Ag

5 EXTRA HOMEWORK 1F 1. Indicate the isotope in each pair that is most likely to be radioactive. (a) 15 O or 16 O (b) 19 F or 20 F (c) 100 Sn or 120 Sn 2. Radioactive 110 Ag with a half-life of 24 seconds is used by forensic scientists to identify trace amounts of the element in bullet lead. How many seconds will it take for the radioactivity of a 110 Ag sample to fall to 3.125% of its original intensity? 3. The age of a rock was to be determined by 238 U dating. 238 U has a half-life of 4.5 x 10 9 years, and eventually decays into stable 206 Pb. If a sample of rock shows that 50% of its 238 U had been converted into 206 Pb, how old is the rock? 4. What is the most massive element produced by fusion in stars? *5. The equation that governs radioactive decay is: n where = n o e - (ln 2 / t 1/2)t n = the final number of radioactive atoms remaining after the decay time, t n o = the initial number of radioactive atoms t 1/2 = the half-life of the radioactive atoms t = the length of time the radioactive atoms have been decaying Radioactive tritium, 3 H, has a half-life of 12.3 years and is used as a tracer in organic chemistry reactions. How many years will it take for the radioactivity to fall to 10.0% of its original intensity?

6 EXTRA HOMEWORK 1G 1. Magnesium has the following stable isotopes: 24 Mg u 78.70% 25 Mg u 10.13% 26 Mg u 11.17% What is the value of the elemental atomic mass for magnesium calculated from these data? 2. The element indium exists in nature as two isotopes: 113 In amu 115 In amu Using the periodic table in your textbook, calculate the natural percentages of the two indium isotopes. 3. Give the mass, in grams, necessary to have one mole of atoms of each of the following elements: (a) beryllium (b) sulfur (c) nickel (d) tin 4. A sample of lead has a mass of 25.0 g. Calculate: (a) the number of moles of lead atoms. (b) the number of atoms of lead. 5. A sample of antimony contains antimony atoms. Calculate: (a) the number of moles of antimony atoms. (b) the number of grams of antimony. *6. A 13 C atom has a mass of u. What is its mass in grams? *7. A regular garden pea has a volume of about 0.5 milliliters. In contrast, the Empire State building has a volume of approximately 1 billion liters. Calculate the number of Empire State Buildings it would take to hold 1 mole of regular garden peas.

7 EXTRA HOMEWORK 1H 1. What was Mendeleev s Periodic Law, and how is it different from the modern Periodic Law. 2. What is similar about elements in the same period on the periodic table? 3. For element 120, Ubn: (a) predict its expected electron configuration notation (b) predict what other element it will most likely resemble chemically 4. Identify the atom with the largest atomic radius, and explain why: (a) Ti, Zr (b) Mn, Fe 5. Identify the atom in each pair with the largest atomic radius: (a) Si, Cl (b) Ca, Ba *6. For element 121, Ubu: (a) predict its expected electron configuration notation (b) predict what other element it will most likely resemble chemically EXTRA HOMEWORK 1I 1. Write the equations for the first, second and third ionizations of an oxygen atom. 2. Identify the atom with the greatest (most endothermic) first ionization energy, and explain why: (a) Ca, Sr (b) S, Cl (c) Be, B (d) Sb, Te 3. Elements X and Y are known to be second or third period elements on the periodic table. The first four ionization energies for elements X and Y are shown below. The units are not kj/mol. Identify elements X and Y. First Second Third Fourth Write the equations for the first, second, and third electron affinities of an oxygen atom. 5. Identify the atom with the greatest (most exothermic) first electron affinity, and explain why: (a) Rb, Cs (b) As, Se (c) Li, Be (d) Sn, Sb (e) C, Si 6. Identify the atom in each pair with (1) the greatest (most endothermic) ionization energy, and (2) the greatest (most exothermic) electron affinity: (a) Si, Cl (b) Ca, Ba *7. Identify the atom with the largest atomic radius, and explain why: (a) K, Mg (b) Co, Cd X Y

8 EXTRA HOMEWORK 1J 1. Give examples of the physical properties of metals and nonmetals. 2. Why do metals form positive ions and nonmetals form negative ions? 3. Give the most metallic element in each pair: (a) K, Ca (b) Sn, Pb 4. Give the charge of the expected ion ion for each of the following elements: (a) I (b) Rb (c) Se (d) Sr (e) As (f) In (g) Cd (h) Fe 5. Give the charges of the two ions expected for each of the following elements: (a) Tl (b) Pb (c) Bi 6. Why do the atoms of Group 1 elements form 1+ ions? 7. Why do the atoms of Group 2 elements form 2+ ions? 8. Why do atoms of the d-sublevel elements form a variety of positive ions? 9. Why do the atoms of Group 17 elements form 1- ions? 10. Why don t the atoms of Group 18 elements form ions? EXTRA 1A ANSWERS 1. Dalton s Atomic Theory explained the Law of Definite Proportion. 2. (a) HO 16, HO 8 (b) HO 2, HO (c) HO, H 2 O 3. (a) discovered the electron (b) discovered the nucleus of the atom cm or 4.5 μm *5. (a) N 2 O, NO, NO 2 (b) N 4 O, N 2 O, NO (c) N 3 O, N 3 O 2, N 3 O 4 *6. (a) 3 g/cm 3 (b) 3 x g/cm 3

9 EXTRA 1B ANSWERS 1. (a) x 10-7 m (b) x s -1 (c) x J (d) x 10 2 kj 2. (a) 3.84 x J (b) 5.79 x s -1 (c) 5.18 x 10-7 m (d) 518 nm (e) visible light *3. light passing through 2 slits produces a diffraction pattern * nm EXTRA 1C ANSWERS 1. values for a property are restricted to multiples of some small, elementary unit 2. (a) (b) (c) x m 4. a diffraction pattern is produced * x m EXTRA 1D ANSWERS 1. (a) forbidden (b) forbidden (c) allowed (d) allowed 2. (a) (b) (c) (d) (continued on next page)

10 3. (a) 4s, 4p, 4d, 4f (b) 4. (a) the 3 rd energy level of an atom (b) the 8 th energy level of an atom (c) the f sublevel in the 4 th energy level of an atom (d) the s sublevel in the 2 nd energy level of an atom, or, the s orbital in the 2 nd energy level of an atom (e) the p orbital on the x axis in the 7 th energy level of an atom (f) the f orbital in the yz 2 space in the 5 th energy level of an atom 5. (a) 32 (b) 200 (c) 10 (d) 2 (e) 2 (f) 2 (g) 2 6. (a) (b) (c) *7. (a) n = 5 (b) 18 *8. (a) 6s, 6p, 6d, 6f, 6g, 6h (b) 36

11 EXTRA BOHR ATOM ANSWERS 1. (a) x J, x J (b) the values are energy of attraction (c) x J (d) energy was released during the process (e) x 10-6 m (f) infrared radiation 2. (a) x J (b) yes, 3.78 x J > x J *3. fourth EXTRA 1E ANSWERS. 1. (a) [Ne]3s 2 3p 2. Si : (b) [Ar]4s 1 3d 5 Cr. (c) [Xe]6s 2 4f 14 5d 10 6p 4. Po :. (d) [Rn]7s 2 5f 6 Pu : 2. 3s 3p x 3p y 3. An electron in a 4s orbital has more probability inside of the inner energy level shielding than an electron in a 3d orbital, so a 4s electron will attract more strongly to the nucleus of the atom than a 3d electron, and therefore an electron in a 4s orbital is more stable than an electron in a 3d orbital 4. (a) excited (b) excited (c) ground (d) impossible 5. (a) 20 p, 20 n, 20 e (b) 23 p, 28 n, 23 e (c) 35 p, 44 n, 36 e (d) 98 p, 154 n, 98 e Th (continued on next page)

12 *7. Electrons in a 2s orbital have more probability inside the shielding of the first energy level electrons than electrons in a 2p orbital, resulting in greater attraction, and therefore a lower energy state. *8. Electrons in a 4s orbital have more probability inside the shielding of the finner energy level electrons than electrons in a 3d orbital, resulting in greater attraction, and therefore a lower energy state. *9. (a) 18 (b) 30 (c) 8 (d) 40 *9. (a) H, Li, B, F, Na, Al, Cl, K, Sc, Cu, Ga, Br (b) C, O, Si, S, Ti, Ni, Ge, Se *10. (a) [Kr]5s 1 4d 5 (b) [Kr]5s 1 4d 10 EXTRA 1F ANSWERS 1. (a) 15 O (b) 20 F (c) 100 Sn seconds x 10 9 years 4. Iron * years EXTRA 1G ANSWERS u 2. 5% 113 In, 95% 115 In 3. (a) g (b) g (c) g (d) g 4. (a) mol (b) 7.27 x atoms 5. (a) mol (b) 5.56 g * x g * billion

13 EXTRA 1H ANSWERS 1. Mendeleev - the properties of the chemical vary with their atomic masses in a systematic way. Modern - the properties of the chemical vary with their atomic numbers in a systematic way. 2. Atoms of the elements in the same period require the same number of energy levels to hold all of their electrons (they all have the same number of energy levels). 3. (a) [Uno]8s 2 (b) Ra 4. (a) Zr - The atomic radius of Zr is greater because the number of shielding energy levels is more than Ti, even though the nuclear charge is greater, so electrons in the highest occupied energy level are less attracted to the nucleus. (b) Mn The atomic radius of Mn is greater because its nuclear charge is less than that of Fe while the number of shielding energy levels remains the same, so electrons in the higheset occupied energy level are less attracted to the nucleus. 5. (a) Si (b) Ba *6. (a) [Uno]8s 2 5g 1 (b) Ac

14 EXTRA 1I ANSWERS 1. O(g) O + (g) + e - O + (g) O 2+ (g) + e - O 2+ (g) O 3+ (g) + e - 2. (a) Ca - The ionization energy of Ca is greater because the number of shielding energy levels is less than Sr, even though the nuclear charge is less, so electrons in the highest occupied energy level are more attracted to the nucleus. (b) Cl - The ionization energy of Cl is greater because its nuclear charge is greater than that of S while the number of shielding energy levels remains the same, so electrons in the higheset occupied energy level are more attracted to the nucleus. (c) Be - The removed electron in Be comes from a 2s orbital, while the removed electron in B comes from a 2p orbital. Electrons in 2s orbitals are less shielded from the nuclear charge, so they are attrached more to the nucleus. (d) Sb - The removed electron in Sb is unpaired, while the removed electron in Te is paired. Unpaired electrons experience less electron-electron repulsion, so they are attrached more to the nucleus. 3. X = Mg, Y = Be 4. O(g) + e - O - (g) O - (g) + e - O 2- (g) O 2- (g) + e - O 3- (g) 5. (a) Rb The electron affinity of Rb is greater because the number of shielding energy levels is less than Cs, even though the nuclear charge is less, so free electrons are more attracted to the nucleus. (b) Se - The electron affinity of Se is greater because its nuclear charge is greater than tht of As while the number of shielding energy levels remains the same, so free electrons are more attracted to the nucleus. (c) Li - The electron added to Li goes into a 2s orbital, while the added electron to Be goes into a 2p orbital. Electrons in 2s orbitals are less shielded from the nuclear charge, so they are attrached more to the nucleus. (d) Sn - The added electron to Sn is unpaired, while the added electron to Sb becomes paired. Unpaired electrons experience less electron-electron repulsion, so they are attrached more to the nucleus. (e) Si - In the p-block of the periodic table, adding electrons to small atoms from the second period (like C) results in large electron-electron repulsion, so their electron affinities are slightly less than atoms from the third period (like Si) 6. (a) Cl greater ionization energy, greated electron affinity (b) Ca greater ionization energy, greated electron affinity *7. (a) [Uno]8s 2 5g 1 (b) Ac

15 EXTRA 1J ANSWERS 1. metals lustrous, malleable, ductile, conductors of heat and electricity; nonmetals opposite 2. metals have low ionization energies and low electron affinities, therefore they lose electrons easily (forming positive ions) but it is difficult for them to gain electrons nonmetals have high ionization energies and high electron affinities, therefore it is difficult for them to lose electrons, but they gain electrons easily (forming negative ions) 3. (a) K (b) Pb 4. (a) 1- (b) 1+ (c) 2- (d) 2+ (e) 3- (f) 3+ (g) 2+ (h) forms more than 1 5. (a) 3+, 1+ (b) 4+, 2+ (c) 5+, Group 1 elements have one outershell electron. That electron has a low ionization energy, so it is removed easily. Further electrons are core electrons (from inner energy levels), and they have high ionization energies, so they are difficult to remove. With one electron being removed easily, those atoms form 1+ ions. Group 1 elements have low electron affinities, so they do not gain electrons. 7. Group 2 elements have two outershell electrons. Those two electrons have low ionization energies, so they are removed easily. Further electrons are core electrons (from inner energy levels), and they have high ionization energies, so they are difficult to remove. With two electrons being removed easily, those atoms form 2+ ions. Group 2 elements have low electron affinities, so they do not gain electrons. 8. For the d-sublevel elements, their outershell s electrons have low ionization energies, so they are removed easily. Their inner d electrons also have fairly low ionization energies, so they may be removed as well, forming different ions with higher positive charges. 9. Group 17 elements have one opening for an electron in their outershell electron. The electron affinity to fill that spot is high, so an electron is gained easily. Further electrons would have to go into higher energy levels, and their electron affinities would be very low, so they are difficult to gain. With one electron being gained easily, those atoms form 1- ions. Group 17 elements have high ionization energies, so they do not lose electrons. 10. Group 18 elements have high ionization energies so they do not lose electrons, and low electron affinities so they do not gain electrons.

Note that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?

Note that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom? Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on

More information

Electrons. Unit H Chapter 6

Electrons. Unit H Chapter 6 Electrons Unit H Chapter 6 1 Electrons were discovered by 1. Dalton 2. Lavoisier 3. Proust 4. Mendeleev 6. Rutherford 7. Bohr 8. Schrodinger 9. Dirac 5. Thomson 2 Electrons were discovered by 1. Dalton

More information

Chapter 2 Atoms and the Periodic Table

Chapter 2 Atoms and the Periodic Table Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.

More information

1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on

1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.

More information

Part A. Answer all questions in this part.

Part A. Answer all questions in this part. Part A Directions (1-20): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.

More information

Full file at

Full file at 16 Chapter 2: Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element. a.

More information

Modern Atomic Theory

Modern Atomic Theory Modern Atomic Theory Review of the Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble. 1875 Crooks discovered the electron.

More information

Unit 1 Part 2 Atomic Structure and The Periodic Table Introduction to the Periodic Table UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE

Unit 1 Part 2 Atomic Structure and The Periodic Table Introduction to the Periodic Table UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE PART 2 INTRODUCTION TO THE PERIODIC TABLE Contents 1. The Structure of the Periodic Table 2. Trends in the Periodic Table Key words: group, period, block,

More information

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals

More information

Nucleus. Electron Cloud

Nucleus. Electron Cloud Atomic Structure I. Picture of an Atom Nucleus Electron Cloud II. Subatomic particles Particle Symbol Charge Relative Mass (amu) protons p + +1 1.0073 neutrons n 0 1.0087 electrons e - -1 0.00054858 Compare

More information

MODERN ATOMIC THEORY AND THE PERIODIC TABLE

MODERN ATOMIC THEORY AND THE PERIODIC TABLE C10 04/19/2013 13:34:14 Page 114 CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is

More information

CDO AP Chemistry Unit 5

CDO AP Chemistry Unit 5 1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic

More information

NJCTL.org 2015 AP Physics 2 Nuclear Physics

NJCTL.org 2015 AP Physics 2 Nuclear Physics AP Physics 2 Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?

More information

Nuclear Physics Questions. 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of?

Nuclear Physics Questions. 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? Nuclear Physics Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?

More information

5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.

5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d. 1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added

More information

Chapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation

Chapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Chapter 10: Modern Atomic Theory and the Periodic Table How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy that exhibits

More information

CHEMISTRY - ZUMDAHL 8E CH.7 - ATOMIC STRUCTURE & PERIODICITY.

CHEMISTRY - ZUMDAHL 8E CH.7 - ATOMIC STRUCTURE & PERIODICITY. !! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of

More information

Unit 7. Atomic Structure

Unit 7. Atomic Structure Unit 7. Atomic Structure Upon successful completion of this unit, the students should be able to: 7.1 List the eight regions of the electromagnetic spectrum in the designated order and perform calculations

More information

CHEMISTRY - KIRSS 2E CH.3 - ATOMIC STRUCTURE: EXPLAINING THE PROPERTIES OF ELEMENTS

CHEMISTRY - KIRSS 2E CH.3 - ATOMIC STRUCTURE: EXPLAINING THE PROPERTIES OF ELEMENTS !! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of

More information

HSVD Ms. Chang Page 1

HSVD Ms. Chang Page 1 Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which

More information

Honors Chemistry: Chapter 4- Problem Set (with some 6)

Honors Chemistry: Chapter 4- Problem Set (with some 6) Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of

More information

Test Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay

Test Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay Test Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay Link download full: https://digitalcontentmarket.org/download/test-bank-for-general-chemistry-atoms-f irst-2nd-edition-by-mcmurry-and-fay/

More information

Key Equations. Determining the smallest change in an atom's energy.

Key Equations. Determining the smallest change in an atom's energy. ATOMIC STRUCTURE AND PERIODICITY Matter and Energy Key Equations λν = c ΔE = hν Relating speed of a wave to its wavelength and frequency. Determining the smallest change in an atom's energy. H( λ =R n

More information

Periodic Table Workbook

Periodic Table Workbook Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order

More information

Discovered the electron

Discovered the electron Aubrey High School AP Chemistry 8 Atomic Theory Name Period Date / / 8.0 Prep Problems History of the Atom 1. Describe the contributions of the following scientists and their research to the theory of

More information

Chapter 4 The Structure of the Atom

Chapter 4 The Structure of the Atom Chapter 4 The Structure of the Atom Read pg. 86-97 4.1 Early Theories of Matter The Philosophers Democritus Artistotle - Artistotle s influence so great and the science so primitive (lacking!) his denial

More information

Unit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.

Unit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct. Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct. According to the law of definite proportions, any two samples of water, H2O, A. will be made up

More information

THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table!

THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table! THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table! Development of the Periodic Table! Main Idea: The periodic table evolved over time as scientists discovered more useful ways

More information

Homework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2

Homework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2 Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)

More information

Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies &

Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & electronegativity The Periodic Table What is the periodic

More information

Periods: horizontal rows (# 1-7) 2. Periodicity the of the elements in the same group is explained by the arrangement of the around the nucleus.

Periods: horizontal rows (# 1-7) 2. Periodicity the of the elements in the same group is explained by the arrangement of the around the nucleus. The Modern Periodic Table 1. An arrangement of the elements in order of their numbers so that elements with properties fall in the same column (or group). Groups: vertical columns (#1-18) Periods: horizontal

More information

Organizing the Periodic Table

Organizing the Periodic Table Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements

More information

Made the FIRST periodic table

Made the FIRST periodic table Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing

More information

Reporting Category 1: Matter and Energy

Reporting Category 1: Matter and Energy Name: Science Teacher: Reporting Category 1: Matter and Energy Atoms Fill in the missing information to summarize what you know about atomic structure. Name of Subatomic Particle Location within the Atom

More information

Why all the repeating Why all the repeating Why all the repeating Why all the repeating

Why all the repeating Why all the repeating Why all the repeating Why all the repeating Why all the repeating Why all the repeating Why all the repeating Why all the repeating Patterns What Patterns have you observed in your life? Where to Get Help If you don t understand concepts in chapter

More information

The Periodic Law Notes (Chapter 5)

The Periodic Law Notes (Chapter 5) The Periodic Law Notes (Chapter 5) I. History of the Periodic Table About 70 elements were known by 1850 (no noble gases) but there didn t appear to be a good way of arranging or relating them to study.

More information

CHAPTER 2. Atoms,Elements, Periodic Table

CHAPTER 2. Atoms,Elements, Periodic Table CHAPTER Atoms,Elements, Periodic Table 1 Vocabulary Chemistry Science that describes matter its properties, the changes it undergoes, and the energy changes that accompany those processes Matter Anything

More information

How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas?

How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? EXAMPLE PROBLEM: How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? 1 - Convert 2545 grams of chlorine to moles chlorine using formula weight 2 - Convert moles

More information

BROOKLYN COLLEGE Department of Chemistry. Chemistry 1 Second Lecture Exam Nov. 27, Name Page 1 of 5

BROOKLYN COLLEGE Department of Chemistry. Chemistry 1 Second Lecture Exam Nov. 27, Name Page 1 of 5 BROOKLYN COLLEGE Department of Chemistry Chemistry 1 Second Lecture Exam Nov. 27, 2002 Name Page 1 of 5 Circle the name of your lab instructor Kobrak, Zhou, Girotto, Hussey, Du Before you begin the exam,

More information

The Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism

The Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism Periodic Properties Atomic & Ionic Radius Energy Electron Affinity We want to understand the variations in these properties in terms of electron configurations. The Periodic Table Elements in a column

More information

Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table

Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate

More information

8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37

8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37 Electronic Structure Worksheet 1 Given the following list of atomic and ionic species, find the appropriate match for questions 1-4. (A) Fe 2+ (B) Cl (C) K + (D) Cs (E) Hg + 1. Has the electron configuration:

More information

Name: Date: ChemT1. 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom?

Name: Date: ChemT1. 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom? Name: Date: ChemT1 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom? A. the atom is very small B. the electrons are moving

More information

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol.

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. Teacher Workbooks Science and Nature Series Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. 1 Copyright 23 Teachnology Publishing Company A Division of Teachnology,

More information

Chapter 2: The Structure of the Atom and the Periodic Table

Chapter 2: The Structure of the Atom and the Periodic Table Chapter 2: The Structure of the Atom and the Periodic Table 1. What are the three primary particles found in an atom? A) neutron, positron, and electron B) electron, neutron, and proton C) electron, proton,

More information

Placeholder zeros, even though they aren't SIGNIFICANT, still need to be included, so we know how big the number is!

Placeholder zeros, even though they aren't SIGNIFICANT, still need to be included, so we know how big the number is! 28 A few more math with significant figures examples: 15047 11 0.9876 Placeholder zeros, even though they aren't SIGNIFICANT, still need to be included, so we know how big the number is! Addition: 147.3

More information

Using the Periodic Table

Using the Periodic Table MATH SKILLS TRANSPARENCY WORKSHEET Using the Periodic Table 6 Use with Chapter 6, Section 6.2 1. Identify the number of valence electrons in each of the following elements. a. Ne e. O b. K f. Cl c. B g.

More information

Unit 3: The Periodic Table and Atomic Theory

Unit 3: The Periodic Table and Atomic Theory Name: Period: Unit 3: The Periodic Table and Atomic Theory Day Page # Description IC/HW 1 2-3 Periodic Table and Quantum Model Notes IC 1 4-5 Orbital Diagrams Notes IC 1 14 3-A: Orbital Diagrams Worksheet

More information

Chapter 8. Periodic Properties of the Element

Chapter 8. Periodic Properties of the Element Chapter 8 Periodic Properties of the Element Mendeleev (1834 1907) Ordered elements by atomic mass Saw a repeating pattern of properties Periodic law when the elements are arranged in order of increasing

More information

SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca

SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca 2. Which of the following influenced your answer to number one the most? a. effective nuclear

More information

Notes: Unit 6 Electron Configuration and the Periodic Table

Notes: Unit 6 Electron Configuration and the Periodic Table Name KEY Block Notes: Unit 6 Electron Configuration and the Periodic Table In the 1790's Antoine Lavoisier compiled a list of the known elements at that time. There were only 23 elements. By the 1870's

More information

2008 Brooks/Cole 2. Frequency (Hz)

2008 Brooks/Cole 2. Frequency (Hz) Electromagnetic Radiation and Matter Oscillating electric and magnetic fields. Magnetic field Electric field Chapter 7: Electron Configurations and the Periodic Table Traveling wave moves through space

More information

Atomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry

Atomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry Atomic Structure Atomic Emission Spectra and Flame Tests Flame Tests Sodium potassium lithium When electrons are excited they bump up to a higher energy level. As they bounce back down they release energy

More information

Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry) Chapter 2 Atoms and the Periodic Table

Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry) Chapter 2 Atoms and the Periodic Table Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry) Chapter 2 Atoms and the Periodic Table 1) The smallest amount of an element that retains that element's characteristics is the A)

More information

1 Arranging the Elements

1 Arranging the Elements CHAPTER 12 1 Arranging the Elements SECTION The Periodic Table BEFORE YOU READ After you read this section, you should be able to answer these questions: How are elements arranged on the periodic table?

More information

Honors Chemistry Unit 4 ( )

Honors Chemistry Unit 4 ( ) Honors Chemistry Unit 4 (2017-2018) Families (research and present) Metals/nonmetals Trends o Atomic radius o Electronegativity o Ionization energy o Metallic and nonmetallic character Review Ions Oxidation

More information

Activity # 2. Name. Date due. Assignment on Atomic Structure

Activity # 2. Name. Date due. Assignment on Atomic Structure Activity # 2 10 Name Date Date due Assignment on Atomic Structure NOTE: This assignment is based on material on the Power Point called Atomic Structure, as well as pages 167-173 in the Science Probe textbook.

More information

CHEMISTRY 110 EXAM 1 SEPTEMBER 20, 2010 FORM A

CHEMISTRY 110 EXAM 1 SEPTEMBER 20, 2010 FORM A CHEMISTRY 110 EXAM 1 SEPTEMBER 20, 2010 FORM A 1. What are the correct numbers of protons, neutrons and electrons in a 39 K + ion? p n e A. 20 19 18 B. 20 19 19 C. 19 20 18 D. 19 20 19 E. 20 19 20 2. Which

More information

- Dalton's theory sets LIMITS on what can be done with chemistry. For example:

- Dalton's theory sets LIMITS on what can be done with chemistry. For example: 34 - Dalton's theory sets LIMITS on what can be done with chemistry. For example: Chemistry can't convert lead (an element) into gold (another element). Sorry, alchemists! You can't have a compound form

More information

CHEM 172 EXAMINATION 1. January 15, 2009

CHEM 172 EXAMINATION 1. January 15, 2009 CHEM 17 EXAMINATION 1 January 15, 009 Dr. Kimberly M. Broekemeier NAME: Circle lecture time: 9:00 11:00 Constants: c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J x s J = kg x m /s Rydberg Constant = 1.096776 x

More information

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass 1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the

More information

SCH3U- R. H. KING ACADEMY ATOMIC STRUCTURE HANDOUT NAME:

SCH3U- R. H. KING ACADEMY ATOMIC STRUCTURE HANDOUT NAME: Particle Theory of Matter Matter is anything that has and takes up. All matter is made up of very small. Each pure substance has its of particle, from the particles of other pure substances. Particles

More information

A. 24 B. 27 C. 30 D. 32 E. 33. A. It is impossible to tell from the information given. B. 294 mm C. 122 mm D. 10 mm E. 60 mm A. 1 H B. C. D. 19 F " E.

A. 24 B. 27 C. 30 D. 32 E. 33. A. It is impossible to tell from the information given. B. 294 mm C. 122 mm D. 10 mm E. 60 mm A. 1 H B. C. D. 19 F  E. CHEMISTRY 110 EXAM 1 Sept. 24, 2012 FORM A 1. A microwave oven uses 2.45! 10 9 Hz electromagnetic waves to heat food. What is the wavelength of this radiation in mm? A. It is impossible to tell from the

More information

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table

Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Name /87 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statements by changing

More information

Lecture Presentation. Chapter 8. Periodic Properties of the Element. Sherril Soman Grand Valley State University Pearson Education, Inc.

Lecture Presentation. Chapter 8. Periodic Properties of the Element. Sherril Soman Grand Valley State University Pearson Education, Inc. Lecture Presentation Chapter 8 Periodic Properties of the Element Sherril Soman Grand Valley State University Nerve Transmission Movement of ions across cell membranes is the basis for the transmission

More information

Chem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00

Chem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00 Chem 1711 Exam 1 September 26, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 N A = 6.022 x 10 23 mol 1 I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gases 1 H 1.008 3 Li

More information

THE STRUCTURE OF ATOMS. ATOMS Atoms consist of a number of fundamental particles, the most important ones are...

THE STRUCTURE OF ATOMS. ATOMS Atoms consist of a number of fundamental particles, the most important ones are... Atomic Structure THE STRUCTURE OF ATOMS ATOMS Atoms consist of a number of fundamental particles, the most important ones are... Mass / kg Charge / C Relative mass Relative Charge PROTON NEUTRON ELECTRON

More information

SCH4U1 Atomic & Molecular Structure Test Review

SCH4U1 Atomic & Molecular Structure Test Review SCH4U1 Atomic & Molecular Structure Test Review 1. Which object(s) would you use to describe the shape of the 2p orbital? a. a dumb-bell b. a circle c. a sphere d. two perpendicular dumb-bells e. a doughnut

More information

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass 1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the

More information

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name:

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name: Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice

More information

Atoms and the Periodic Table

Atoms and the Periodic Table Atoms and the Periodic Table Parts of the Atom Proton Found in the nucleus Number of protons defines the element Charge +1, mass 1 Parts of the Atom Neutron Found in the nucleus Stabilizes the nucleus

More information

Atomic structure. The subatomic particles. - a small, but relatively massive particle that carres an overall unit POSITIVE CHARGE

Atomic structure. The subatomic particles. - a small, but relatively massive particle that carres an overall unit POSITIVE CHARGE 35 Atomic structure - Until the early 20th century, chemists considered atoms to be indivisible particles. - The discovery of SUBATOMIC PARTICLES changed the way we view atoms! PROTON NEUTRON ELECTRON

More information

1. Ham radio operators often broadcast on the 6 meter band. The frequency of this electromagnetic radiation is MHz. a. 500 b. 200 c. 50 d. 20 e. 2.

1. Ham radio operators often broadcast on the 6 meter band. The frequency of this electromagnetic radiation is MHz. a. 500 b. 200 c. 50 d. 20 e. 2. Name: Score: 0 / 60 points (0%) [1 open ended question not graded] Chapters 6&7 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Ham radio

More information

Atomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.

Atomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the atomic

More information

Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass

Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following

More information

The Periodic Table of the Elements

The Periodic Table of the Elements The Periodic Table of the Elements All matter is composed of elements. All of the elements are composed of atoms. An atom is the smallest part of an element which still retains the properties of that element.

More information

4.1 Atomic structure and the periodic table. GCSE Chemistry

4.1 Atomic structure and the periodic table. GCSE Chemistry 4.1 Atomic structure and the periodic table GCSE Chemistry All substances are made of atoms this is cannot be chemically broken down it is the smallest part of an element. Elements are made of only one

More information

Atomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons?

Atomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons? Name Chemistry Atomic Structure Essential Question: How was the structure of the atom determined? Vocabulary: bright-line spectrum electron configuration excited state ground state orbital wave-mechanical

More information

How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas?

How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? 146 EXAMPLE PROBLEM: How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? 1 - Convert 2545 grams of chlorine gas to moles. Use formula weight. 2 - Convert moles

More information

UNIT (2) ATOMS AND ELEMENTS

UNIT (2) ATOMS AND ELEMENTS UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called

More information

Unit 02 Review: Atomic Theory and Periodic Table Review

Unit 02 Review: Atomic Theory and Periodic Table Review Practice Multiple Choice Questions Unit 02 Review: Atomic Theory and Periodic Table Review 1. The number of neutrons in an atom of radioactive C 14 is: a) 6 c) 8 b) 12 d) 14 2. When a radioactive nucleus

More information

A little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table?

A little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table? ü // A little history Johahann Dobereiner (80-89) o Triads John Newlands (8-898) o Law of Octaves Who put together the first useable ic Table? Mendeleev you remember him right? When and How? You know it

More information

KWL CHART--ELECTRONS

KWL CHART--ELECTRONS KWL CHART--ELECTRONS WHAT DO I ALREADY KNOW ABOUT ELECTRONS? WHAT DO I WANT TO KNOW CONCERNING ELECTRONS? WHAT HAVE I LEARNED TODAY ABOUT ELECTRONS? GPS STANDARD SC3. Students will use the modern atomic

More information

Putting it together... - In the early 20th century, there was a debate on the structure of the atom. Thin gold foil

Putting it together... - In the early 20th century, there was a debate on the structure of the atom. Thin gold foil 36 Putting it together... - In the early 20th century, there was a debate on the structure of the atom. RUTHERFORD EXPERIMENT Where do the particles go? Radioactive material A few bounce back A few particles

More information

Review 6: Modern Atomic Theory. Copyright Cengage Learning. All rights reserved. 11 1

Review 6: Modern Atomic Theory. Copyright Cengage Learning. All rights reserved. 11 1 Review 6: Modern Atomic Theory Copyright Cengage Learning. All rights reserved. 11 1 The concept of the nuclear atom left unanswered questions about 1. why the nucleus is so dense. 2. why the negative

More information

ใบงานว ชาเคม 1 (Chemistry Worksheets)

ใบงานว ชาเคม 1 (Chemistry Worksheets) อะตอมและตารางธาต เคม ม.4 1 ใบงานว ชาเคม 1 (Chemistry Worksheets) เร อง อะตอมและตารางธาต () ของ เลขท ห อง สอนโดย คร อ งคาร เทพร ตนน นท สาน กงานเขตพ นท การศ กษาม ธยมศ กษา เขต 11 โรงเร ยนสวนศร ว ทยา จ งหว

More information

9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom)

9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom) CAPTER 6: TE PERIODIC TABLE Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom) The Periodic Table (Mendeleev) In 1872, Dmitri

More information

Chemistry (

Chemistry ( Question 2.1: (i) Calculate the number of electrons which will together weigh one gram. (ii) Calculate the mass and charge of one mole of electrons. Answer 2.1: (i) Mass of one electron = 9.10939 10 31

More information

Unit 3. Atoms and molecules

Unit 3. Atoms and molecules Unit 3. Atoms and molecules Index. s and compounds...2.. Dalton's Atomic theory...2 2.-The atom...2 3.-Atomic number and mass number...2 4.-Isotopes, atomic mass unit and atomic mass...3 5.- configuration...3

More information

Chapter 9: Electrons and the Periodic Table

Chapter 9: Electrons and the Periodic Table C h e m i s t r y 1 2 C h 9 : E l e c t r o n s a n d P e r i o d i c T a b l e P a g e 1 Chapter 9: Electrons and the Periodic Table Work on MasteringChemistry assignments What we have learned: Dalton

More information

Periodic Trends. 1. Why is it difficult to measure the size of an atom? 2. What does the term atomic radius mean? 3. What is ionization energy?

Periodic Trends. 1. Why is it difficult to measure the size of an atom? 2. What does the term atomic radius mean? 3. What is ionization energy? Periodic Trends 1. Why is it difficult to measure the size of an atom? 2. What does the term atomic radius mean? 3. What is ionization energy? 4. What periodic trends exist for ionization energy? 5. What

More information

Chapter 2: Atoms and the Periodic Table

Chapter 2: Atoms and the Periodic Table 1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above is a metal. Ans: A Difficulty:

More information

- Why are phase labels required? Because phase changes either absorb or release energy. ... what does this mean?

- Why are phase labels required? Because phase changes either absorb or release energy. ... what does this mean? 157 SINCE the enthalpy change does NOT depend on path, this means that we can use standard values for enthalpy to predict the heat change in reactions that we have not tested in a calorimeter. THERMOCHEMICAL

More information

Test Review # 4. Chemistry: Form TR4-9A

Test Review # 4. Chemistry: Form TR4-9A Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels

More information

6.3 Classifying Elements with the Periodic Table

6.3 Classifying Elements with the Periodic Table 6.3 Classifying Elements with the Periodic Table The Periodic Table was developed by scientists to organize elements in such a way as to make sense of the growing information about their properties. The

More information

Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1

Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1 Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1 The development of the periodic table brought a system of order to what was otherwise an collection of thousands of pieces of information.

More information

Atoms and The Periodic Table

Atoms and The Periodic Table Atoms and The Periodic Table A. Early Models of the Atom 1. The earliest models of the atom came in the 5 th century B.C. when In the 4 th century, B.C., rejected this idea and proposed that earthly matter

More information

Ch. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements.

Ch. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements. Ch. 3 Answer Key 1. The Greeks believed that all matter is made of elements. We currently believe the same thing. However, the Greeks believed that there were 4 elements: earth, water, air and fire. Instead,

More information

NUCLEAR MODEL. Electron cloud. Electron cloud. Nucleus. Nucleus

NUCLEAR MODEL. Electron cloud. Electron cloud. Nucleus. Nucleus 37 NUCLEAR MODEL - Atoms are mostly empty space - NUCLEUS, at the center of the atom, contains protons and neutrons. This accounts for almost all the mass of an atom - Electrons are located in a diffuse

More information