5. Name three characteristics of most metalloids. Semiconductors of electricity, solid at room temperature, less malleable that metals.
|
|
- Dylan Hodges
- 6 years ago
- Views:
Transcription
1 Chemistry Honors Semester 1 Final Review 1. Classify each of the following as a physical or chemical change: ice melting physical paper burning chemical Acid reacting with oxygen chemical gas under pressure physical liquid evaporating physical Magnesium being heated chemical 2. What is a chemical change and what is a physical change? A chemical change involves a rearrangement of the elements in a substance to form substances with different physical properties. A physical change may change the state of a substance will not change the composition of that substance. 3. Name three characteristics of most nonmetals. Brittle, low electrical and thermal conductivity, low boiling point 4. Name three characteristics of metals. Malleable, ductile, good conductors of heat and electricity, luster. 5. Name three characteristics of most metalloids. Semiconductors of electricity, solid at room temperature, less malleable that metals. 6. Name two properties of noble gases. Generally unreactive, gas at room temperature. 7. Consider the burning of gasoline and the evaporation of gasoline. Which process represents a chemical change and which represents a physical change? Give a reason for you answer. The burning of gasoline represents a chemical change because the gasoline is being changed into substances with different identities, Evaporation involves a physical change; the identity of gasoline remains unchanged. 8. Report the number of significant figs in each of the following values g J 3 64 ml x 10 2 cm x 10 2 cm Round the following top 3 significant figures: 22.77g 22.8g m 14.6 m L 9.53 L cm 87.6 cm g 30.3
2 10. Three students were asked to determine the volume of a liquid by a method of their choosing. Each did three trials.. The table below shows results. ( The actual volume is 24.8 ml.) Trial (ml) Trial 2 (ml) Trial 3 (ml) Student A Student B Student C a.) Which students measurements showed greatest accuracy? Student C b.) Which students measurements showed the greatest precision? Student C and B (correction in table) 11. A single atom of platinum has a mass of 3.25 X g. What is the mass of 6.0 X platinum atoms? 2.0 X 10 2 g. 12. A sample thought to be pure lead occupies a volume of 15.0 ml and has a mass of 160.0g. a.) determine its density g/ml g of baking soda, NaHCO 3,, always contains 22.99g of sodium, 1.01g of hydrogen, 12.01g of carbon, and 48.00g of oxygen. What percentage by mass of each of these elements is present in baking soda? Element Percentage Element Percentage sodium 27.37% carbon 14.30% hydrogen 1.20% oxygen 57.14% a. Which law do these data illustrate? The law of definite proportions 14. The smallest unit of an element hat can exist either alone or in combination with atoms of the same or different element is the atom 15.. A positively charged particle found in the nucleus is called a(n) proton 16.. A nuclear particle that has no electrical charge is called a(n) neutron 17.. The subatomic particles that are least massive and most massive, respectively, are the electron and neutron 18.. A cathode ray produced in a gas-filled tube moves away from a negative field, such as one produced by a magnet. When a paddle wheel is installed inside the tube, the wheel moves down the tube in the same direction as the cathode ray. What properties of electrons do these two phenomena illustrate? Who did this experiment? - electrons has charge and mass. Thompson 19. How would the electrons produced in a cathode ray tube filled with neon gas compare with the electrons produced in a cathode ray tube filled with chlorine gas? - The electrons produced from neon gas and chlorine gas would behave in the same way because electrons do not differ from element to element. 20. Explain the difference between the mass number and the atomic number of a nuclide. - Mass number is the total number of protons and neutrons in the nucleus of an isotope. Atomic number is the total number of protons only in the nucleus of each atom of an element.
3 21. How many particles are in 1 mole of carbon? 1 mol of lithium? 1 mol of eggs? Will 1 mol of each of these substances have the same mass? There are x particles in 1 mol of each of these substances. A mole of each substance will not have the same mass. 22. As the atomic masses of the elements in the periodic table increase, what happens to each of the following: a. the number of protons increases b. the number of electrons increases c. the number of atoms in 1 mol of each element stays the same 23. What is the mass in grams of 2 mol of oxygen atoms? _32.00g 24 The element boron, B, has an atomic mass of amu according to the periodic table. However, no single atom of boron has a mass of exactly 10.81amu. How can you explain this difference? The periodic table reports the average atomic mass, which is a weighted average of all isotopes of boron. 25. How did the outcome of Rutherford s gold foil experiment indicate the existence of a nucleus? - The particles rebounded, and therefore must have hit a dense bundle of matter. Because such a small percentage of particles were redirected he reasoned that this clump of matter, called the nucleus, must occupy only a small fraction of the atoms total space. 26. A certain element exists as three natural isotopes as shown in the table below: Isotope Mass (amu) Percent natural abundance Mass number Calculate the average atomic mass of this element amu 27. What is the difference between the ground state and the excited state of an atom (its electrons)? - In order for an electron to be ejected from a metal surface, the electron must be struck by a single photon with at least the minimum energy needed to knock the electron loose. 28. The wavelength of light is 310nm. Calculate its frequency. _9.7 x Hz 29. What is the wavelength of electromagnetic radiation if its frequency is 3.2x 10-2 Hz.? 9.4 x 10 9 m 30. Compare and contrast Hund s rule with the Pauli exclusion principle. 31. Explain the conditions under which the following orbital notation for helium is possible: This orbital notation is possible if an electron in helium s orbital has been excited. 1s 2s 32. Write the electron configuration and orbital diagrams for each of the following atoms: a Phosphorus: 1s 2 2s 2 2p 6 3s 2 2p 3 b b 1s 2s 2 px 2 py 2 pz 3s 3px 3py 3pz b Nitrogen 1s 2 2s 2 2p 3 1s 2s 2 px 2 py 2 pz
4 33. Write the electron configuration of the following atoms: a. Carbon 1s 2 2s 2 2p 2 b copper 1s 2 2s 2 2p 6 3p 6 4s 1 3d What would be the wavelength of light that has a frequency of 3 x 10-4 Hz in a vacuum? 1 x m 35 When an electron is added to a neutral atom, energy is C_ (a) always absorbed (c)either absorbed or released (d) always released (d)burned away 36. The energy required to remove an electron from an atom is the atom s D (a) electron affinity (c)electro negativity (b)electron energy (d) ionization energy 37. Moving from left to right across a period on the periodic table. a. electron affinity values tend to become (more negative or more positive) _more negative b. ionization energy values tend to become (larger or smaller) _larger c. atomic radii tend to become (larger or smaller) _smaller 38. a. Name the halogen with the least negative electron affinity. _At _ b. Name the alkali metal with the highest ionization energy Li _ c. Name the element in Period 3 with the smallest atomic radius. _Ar _ d. Name the Group 14 element with the largest electro negativity. _C _ 39 a. Compare the size of the radius of a positive ion to its neutral atom. In positive ions, the radius is smaller than its corresponding neutral atom. b. Compare the size of the radius of a negative ion to its neutral atom. In negative ions, the radius is larger than its corresponding neutral atom 40. For metals and nonmetals, which tend to form positive ions? Which tend to form negative ions? Metals tend to form positive ions; nonmetals tend to form negative ions 41. Explain the role of valence electrons in the formation of chemical compounds. Valence electrons are the electrons most subject to the influence of nearby atoms or ions. They are the electrons available to be lost, gained, or shared in the formation of chemical compounds 42. Consider a neutral atom with 53 protons and 74 neutrons to answer the following questions. a. What is atomic number? 53 b. What is the mass in amus? 127 amu c. Is the element s position in a modern periodic table determined by its atomic number or by its atomic mass? atomic number 43. Consider an element whose outermost electron configuration is 3d 10 4s 2 4p x a. To which period does the element belong? Period 4 b. If it is a halogen, what is the value of x? _5 c. The group number will equal (10+2+x). True or false? _ true 44.. a. Metalloids are found in which block, s,p,d, or f? p
5 b. The hardest, densest metals are found in which block, s, p, d, or f? d 45. Referring only to the periodic table, answer the following questions on periodic trends. a. Which has the larger radius, Al or ln? _ ln b. Which has the larger radius, Se or Ca? _Ca c. Which has a larger radius, Ca or Ca 2++?_Ca d. Which has greater ionization energies as a class, metals or nonmetals? _nonmetals e. Which has the greater ionization energy, As or Cl? _Cl f. an element with a large negative electron affinity is most likely to form a positive ion, a negative ion, or a neutral atom? _negative ion 46. Explain why ionic bonds tend to form between metals and nonmetals. Ionic bonds form between elements with electronegativity differences greater than 2.0. Metals tend to have low electronegativity while nonmetals have high electronegativity. Metals will more easily give up electrons to nonmetals, whose atoms are more likely to accept electrons. 47. Explain why the formula of glucose is written as C 6 H 12 O 6 and not as CH 2 O. The formula of glucose is written as C 6 H 12 O 6 and not as CH 2 O because a molecule of glucose contains 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms 48. What do the letters VSEPR stand for? Explain what the theory says and how it is used. VSEPR stands for valence-shell electron pair repulsion. The theory states that, in small molecules, pairs of valence electrons are arranged as far apart as possible. The theory is used to account for molecular shapes. 49. Explain why silicon tetrafluoride (SiF 4 ) has a square structural formula but a tetrahedral arrangement in space. The structural formula is a two-dimensional representation and does not take into account the availability of the space above and below the plane of the molecule. If the atoms were arranged in a planar square, the bond angles would be 90, but in the tetrahedral orientation (the correct one) the angles are 109.5, a wider and more desirable separation of electrons. 50. A scientist is plotting the location of the bonding electrons in vaporized beryllium hydride (BeH 2 ) molecules. On the basis of beryllium's electron configuration, she expects the graph to show a spherical s orbital that beryllium shares with one hydrogen and a dumbbell-shaped p orbital that beryllium shares with the other hydrogen. She also expects one bond to be shorter than the other because of the different kinds of orbitals. Describe what the scientist will actually find. Hybridization of the s and the p orbitals of beryllium occurs so that two sp orbitals result. Thus, a dumbbell-shaped probability distribution will be observed rather than the shapes characteristic of separate s and p orbitals. Thus, the two bonds will be equal in length because of the equivalence of the two sp orbitals 51. How many valence electrons does the sulfide ion have? The sulfur atom? The sulfide ion has 8 valence electrons and the sulfur atom has 6 valence electrons 52 How many valence electrons are in the polyatomic ion HPO 4 2? phosphate ion has 32 valence electrons (1 from hydrogen, 5 from the phosphorous, 24 from the four oxygen atoms, and 2 from the 2 charge).
6 53. How many electrons are shared among carbon atoms in the compound ethanol, CH 3 CH 2 OH? Two electrons are shared among the carbon atoms in ethanol 54 Sulfur is the central atom in sulfur dichloride, SCl 2. What is the shape of this molecule? What are the approximate bond angles? In SCl 2, sulfur is connected to each chlorine by a single bond and also has two unshared electron pairs. According to VSEPR, the shape should be bent, and the unshared pairs should reduce the bond angle to about Describe the shape for a molecule of silane, SiH 4. In SiH 4, silicon is connected to each hydrogen atom by a single bond and has no unshared pairs. According to VSEPR, the molecule should be tetrahedral and the bond angles about What is the shape of a molecule of nitrosyl chloride, NOCl, given that nitrogen is the central atom? What are the bond angles? The nitrogen atom forms 3 bonds., the oxygen :two bonds, & chlorine atom one bond. N is central atom, there must be a single bond between nitrogen and chlorine and a double bond between nitrogen and oxygen. Nitrogen also has an unshared electron pair. Keeping the oxygen, chlorine, and unshared pair of electrons a maximum distance apart requires a trigonal planar electron-pair geometry and a bent shape. The bond angle is approximately A molecule has boron as its central atom and two chlorine atoms and one iodine atom, each connected by a single bond to boron. Determine if the molecule is polar, given the following electronegativities: B, 2.0; I, 2.5; and Cl, 3.0. Each bond is polar, with boron at the positive end of each. The molecule is trigonal planar, but in this molecule the polarities do not cancel because the chlorines are more electronegative than the iodine. The molecule as a whole is polar, with the chlorine end having a slightly negative charge. 58. Fill in the following table with the correct name or formula: Name Binary, Ternary or Molecular Formula Beryllium Chloride Binary BeCl 2 Iodine Heptafluoride Molecular IF 7 Chromium (III) nitrite Ternary Cr(NO 2 ) 3 Chlorine Trifluoride Molecular ClF 3 Diphosphorus trioxide Molecular P 2 O 3 Calcium acetate Ternary Ca(C 2 H 3 O 2 ) A compound has the empirical formula NO 2. Its molecular formula could be: a a. NO 2. b. N 2 O. c. N 4 O 2. d. N 4 O A compound consists of 85 percent silver and 15 percent fluorine by mass. What is its empirical formula? AgF
Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom
Semester Review What happens to electronegativity down a group? electrons for aluminum Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom Circle
More informationA sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature.
Semester Review A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature. 1.83 g/l Describe what defines an element s
More informationChapter 4 Atoms Practice Problems
Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a
More information5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons
1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly
More informationCh. 1: Introduction to Chemistry. Ch. 2: Matter and Change
Review Sheet for Chemistry First Semester Final Refer to your class notes, worksheets, and the textbook to complete this review sheet. Study early so that you will have time to ask questions about what
More informationChemistry 1-2E Semester I Study Guide
Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound
More informationUnit 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 informationPeriodic 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 informationLesson 6: Periodic Table & Atomic Theory
Lesson 6: Periodic Table & Atomic Theory Do Now 7Hg 10.11.18 In CJ, copy info down from board. Keep CJs out and open on your desk. On Do Now page, copy and answer questions below. 1. Name 4 properties
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationChemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
More informationTest 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 informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationLesson 6: Periodic Table and Atomic Theory
NOTES Name: _ Date: Class: Lesson 6: Periodic Table and Atomic Theory Element: fundamental substance that ; all matter consists of ~100 elements Atom: _ that can exist; smallest unit of an element that
More informationIonic Bonding Ionic bonding occurs when metals and nonmetals trade one or more electrons and the resulting opposite charges attract each other. Metals
Chemical Bonding Now that we know what atoms look like A very small (less than 0.001% of the volume) and massive (more than 99.99% of the mass) nucleus with protons (+) and neutrons (neutral) and electrons
More informationLab safety and equipment: Sig Figs and Metric Conversions. Matter. Chemistry Review
Lab safety and equipment: Chemistry Review Know: How to handle chemicals and laboratory equipment safely. Basic laboratory equipment Sig Figs and Metric Conversions Significant Figures How many significant
More informationLab safety and equipment: Sig Figs and Metric Conversions. Matter. Chemistry Review
Lab safety and equipment: Chemistry Review Know: How to handle chemicals and laboratory equipment safely. Basic laboratory equipment Sig Figs and Metric Conversions Significant Figures How many significant
More informationFALL SEMESTER REVIEW NAME: PERIOD: 3. (Unit 2) Is the following picture representing accuracy, precision or both? Explain the difference.
FALL SEMESTER REVIEW NAME: PERIOD: 1. (Unit 7) When the equation Cu + AgNO 3 Cu(NO3) 2 + Ag is balanced the coefficient of Ag NO 3 is? 2. (Unit 7) Balance the following equation: AgNO 3 + BaCl 2 AgCl +
More informationSecond Semester Chemistry Study Guide
Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on
More informationAE Chemistry Midterm Study Guide
Name Date Define Chemistry AE Chemistry Midterm Study Guide Since chemistry studies matter what is the definition of matter. What is the Law of Conservation of Matter? What is energy, what are the two
More informationTest 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 informationUnit 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 informationMemorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
More informationHonors 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 informationHomework 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 informationName: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
More informationClassify 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 informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationChemistry Mid-Term Exam Review Spring 2017
Unit 1 Measurement & Math Accuracy & Precision (recognizing given lab data) Density calculations Number of SFs in a measurement, Round answers to correct number of SFs Percent Error Unit conversions in
More informationModern 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 informationName Midterm Review Date
Name Midterm Review Date 1. In which process does a solid change directly into a vapor? A) sublimation B) deposition C) condensation D) solidification 2. What is the molecular formula of a compound that
More informationPeriodic Table Practice 11/29
Periodic Table Practice 11/29 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
More informationMultiple Choice Identify the choice that best completes the statement or answers the question.
Covalent Practice CP November 2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Bromine, atomic number 35, belongs to Group 17. How many electrons does
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM 210 Chemistry Homework #2 Atoms and Elements (Ch. 3) Due: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Helium is a(n) A) heterogeneous mixture.
More informationChemistry Final Review 2017
Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,
More informationUnit 3 Periodic Table and Quantum HW Packet Name Date. Periodic Table Concepts. 1. In what family are the most active metals located?
Directions: Answer the following questions. Periodic Table Concepts 1. In what family are the most active metals located? 2. In what family are the most active non-metals located? 3. What family on the
More informationCP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B.
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B. kilo D. deka E. deci G. milli H. micro C. hecto
More informationName Date Period Chemistry Final Exam Review Packet - Fall 2014
Name Date Period Chemistry Final Exam Review Packet - Fall 2014 Periodic Table and Atomic Structure Physical properties can be intensive or extensive. Intensive properties do not change with amount of
More information3.1 Classification of Matter. Copyright 2009 by Pearson Education, Inc.
Chapter 3 Atoms and Elements 3.1 Classification of Matter Copyright 2009 by Pearson Education, Inc. 1 Matter Matter is the stuff that makes up all things. Copyright 2009 by Pearson Education, Inc. 2 Pure
More informationAtomic Structure. Ch 3 Prentice Hall
Atomic Structure Ch 3 Prentice Hall The Nuclear Atom By 1919 Rutherford concluded that the atom has a dense positive center called the nucleus containing what he called protons The electrons surround
More informationPeriod: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?
Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States
More informationMIDTERM STUDY GUIDE. Chapter 1 Introduction to Chemistry
MIDTERM STUDY GUIDE Chapter 1 Introduction to Chemistry What is chemistry? Chemical properties vs. physical properties examples of both States of matter Scientific method Chapter 2 Data Analysis SI measurement
More informationChapter 6 Chemistry Review
Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in
More information4. Draw a concept map showing the classifications of matter. Give an example of each.
Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.
More informationLab safety and equipment: Sig Figs and Metric Conversions. Matter. Chemistry Review
Lab safety and equipment: Chemistry Review Know: How to handle chemicals and laboratory equipment safely. Basic laboratory equipment Sig Figs and Metric Conversions Significant Figures How many significant
More information1. 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 information2. What is the energy of a single photon of blue light with a wavelength of 4.50 x 10-7 m?
2013 Chemistry Fall Exam Review Concepts to review/explain: 1. Using the periodic table, what is the electron configuration for Sulfur, Calcium and Copper? 2. What is the energy of a single photon of blue
More informationAtomic Structure Chapter 5 Assignment & Problem Set
Atomic Structure Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Atomic Structure 2 Study Guide: Things You Must Know Vocabulary (know the definition
More informationQuestions 1 to 58 must be answered on the Scantron sheets.
Questions 1 to 58 must be answered on the Scantron sheets. Base your answers to questions 1 to 5 on the heating curve for a pure substance that is shown below. 1. The freezing point of the substance is
More informationChapter 3: Electron Structure and the Periodic Law
Chapter 3: Electron Structure and the Periodic Law PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form the statement is:
More informationVolume of water g g? 50.0 ml ?
MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm
More informationNote 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 informationChapter Test B. Chapter: Arrangement of Electrons in Atoms. possible angular momentum quantum numbers? energy level? a. 4 b. 8 c. 16 d.
Assessment Chapter Test B Chapter: Arrangement of Electrons in Atoms PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
More informationTeacher: Mr. gerraputa. Name: Base your answer to the question on the information below. Given the electron dot diagram:
Teacher: Mr. gerraputa Print Close Name: 1. Given the electron dot diagram: The valence electrons represented by the electron dot diagram could be those of atoms in Group 1. 13 3. 3 2. 15 4. 16 2. Which
More informationDirections: Please choose the best answer choice for each of the following questions.
Directions: Please choose the best answer choice for each of the following questions. 1. Kevin is listing the similarities between metallic and ionic bonds for a laboratory project. Which similarity regarding
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More informationAcademic Chemistry 2016 Fall Final Exam Review DUE THE DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on the final exam
Name Teacher Period Academic Chemistry 2016 Fall Final Exam Review DUE THE DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on the final exam Unit 1 Matter and Change 1. Complete the chart. Definite shape? (y/n)
More informationClass Period. 4. What distinguishes a polar covalent bond from a nonpolar covalent bond?
Cut along dotted line. Name Assignment #1 Chemical Bonding (Predicting Bond Types) 1. What is a chemical bond? 2. Why do atoms form chemical bonds? 3. What distinguishes an ionic bond from a covalent bond?
More informationACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET
ACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET 100. Determine the number of significant figures in the following numbers: a. 100 b. 0.000123 c. 1.00300 d. 1.2300 e. 1.20 x 10 16 f..00010100 Write the following
More informationExam Electrons and Periodic Table
1-20 multiple choice. Answer on scantron. 21-25 short response. Answer on exam paper. All questions are 4 points each. 1. Which term is defined as the region in an atom where an electron is most likely
More information2. Read pages a. Answer the five Reading Check questions on page 47
Chemistry Test #1 Review Chapters 1 & 2 1. Page 37, #4-6, 8, 9, 13, 14 2. Read pages 45 47 a. Answer the five Reading Check questions on page 47 3. Read pages 52 57 a. Copy the table on page 55 b. Define
More informationChemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds
Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section
More informationUnit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS Review of Atomic Structure What is an atom? The smallest particle of an element that retains the properties of that
More informationName: Electrons in Atoms Chemical Periodicity Chapters 13 and 14
Name: Electrons in Atoms Chemical Periodicity Chapters 13 and 14 1 Chapter 13 Electrons in Atoms We need to further develop our understanding of atomic structure to help us understand how atoms bond to
More informationChapter 2 Atoms and Elements
Chapter 2 Atoms and Elements Law of Conservation of Mass in a chemical reaction, matter is neither created nor destroyed total mass of the materials you have before the reaction must equal the total mass
More informationCh. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE What Makes Red Light Red? (4.1) Electromagnetic Radiation: energy that travels in waves (light) Waves Amplitude: height
More informationCh. 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 informationCHEMISTRY I - HONORS MIDTERM REVIEW* *Test may cover other topics not included on this review, yet have been covered throughout the semester.
Name Period CHEMISTRY I - HONORS MIDTERM REVIEW* *Test may cover other topics not included on this review, yet have been covered throughout the semester. Chapter 2 Measurement & Calculations Describe the
More informationName: Midterm Review Date:
Name: Midterm Review Date: 1. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) Different elements must have different numbers of neutrons.
More informationName: 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 informationBonding Practice Exam
Bonding Practice Exam Matching Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure
More information5) Which statement correctly describes the relationship of wavelength and frequency in a wave?
Exam 2 Name: Multiple Choice (2 pts each) 1) Which of the following bonds is the most polar? a) C O b) N O c) O O d) Si O 2) The maximum electron capacity of an f sublevel is a) 7 c) 14 b) 6 d) 10 3) Which
More informationOrganizing 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 information11. The bright-line spectra produced by four elements are represented in the diagram below.
1. Which substance can not be broken down by a chemical change? A) ammonia B) ethanol C) propanal D) zirconium 2. Which particle has no charge? A) electron B) neutron C) positron D) proton 3. Which phrase
More informationIn the modern periodic table, elements are arranged by increasing atomic number
THE MODERN PERIODIC TABLE The Periodic Law Q. How is the modern periodic table organized? In the modern periodic table, elements are arranged by increasing atomic number (number of protons). Properties
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:
More informationChapter 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 informationName: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What
More informationAtoms & the Periodic Table. Chapter Outline. Elements
Atoms & the Periodic Table Chapter Outline What is Atom? Chemical properties of Atoms: the Periodicity Isotopes Electrons in Atom: Quantum physics view Valence electrons and the Periodic Table 2 Elements
More informationAtoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2
Name Date Due Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2 Directions: Write your answers to the following questions in the space provided. For problem solving, all of the
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationPeriodic Table of Elements
Periodic Table of Elements chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon Elements Science has come along way since Aristotle s theory of Air, Water, Fire,
More informationCP Chemistry Semester 1 Final Review KEY. Unit 1
CP Chemistry Semester 1 Final Review KEY Unit 1 Practice Problems 1. What tool do you use to measure volume of water? Describe how to make a proper measurement of a volume of water using a 50 ml graduated
More informationnew experimental data, and can be modified
Mass in grams 10 20 30 40 50 Name: Date: Period: CP Chemistry Semester 1 Final Test Review CHAPTERS 1 & 2: Scientific Method, Density, Metric Conversions, Accuracy/Precision, Significant Figures 1. Know
More informationName PRACTICE Unit 3: Periodic Table
1. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have (1) fewer valence electrons (2) more valence electrons (3) fewer electron shells (4) more electron shells 2. On the
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
More information1. 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 informationCHAPTER 6 CHEMICAL BONDING SHORT QUESTION WITH ANSWERS Q.1 Dipole moments of chlorobenzene is 1.70 D and of chlorobenzene is 2.5 D while that of paradichlorbenzene is zero; why? Benzene has zero dipole
More informationCP Chemistry Semester 1 Final Test Review
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega M 10 6 D. deka da 10 1 G. milli m 10 6 B. kilo k
More informationPeriodic Table Practice Questions
Periodic Table Practice Questions 1. Elements in the Periodic Table are arranged according to their (1) atomic number (3) relative activity (2) atomic mass (4) relative size 2. Elements in a given period
More informationPractice Periodic Table Review
Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the
More informationUnits 1, 2 study guide- atomic structure
Name: Units 1, 2 study guide- atomic structure 1) Complete the required information for each subatomic particle (T1.3) symbol name charge location Mass (AMU) p + e - n 0 2) Define the following terms:
More informationQ1. The electronic structure of the atoms of five elements are shown in the figure below.
Q1. The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements. Choose the element to answer the question. Each element can be
More informationChemistry Chapter 6 Test Review
Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons
More informationCHEMISTRY 102 Spring 2013 Hour Exam I Page 1. Which molecule(s) has/have tetrahedral shape and which molecule(s) is/are polar?
Hour Exam I Page 1 1. Consider the following molecules: SiF 4, SeF 4, XeF 4 Which molecule(s) has/have tetrahedral shape and which molecule(s) is/are polar? a) SeF 4 has tetrahedral shape and XeF 4 is
More informationGroups vs. Periods what s the difference?? Groups: Periods:
Before watching the video: Use page 131 in your book or the internet to label the periodic table according to the following guidelines (NOTE: Your key might not look exactly like the book!!!) a. Color
More informationSymbol Atomic Number
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations February Break Review Sheets - /150 Chemistry has a LOT of words. Take this break to review and strengthen your knowledge of the vocabulary you
More informationPart 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