The Atom/Periodic Table After School Regents Review Practice
|
|
|
- Bruno Casey
- 6 years ago
- Views:
Transcription
1 1. An ion that consists of 7 protons, 9 neutrons, and 10 electrons has a net charge of A) 2 B) 2+ C) 3+ D) 3 2. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C) an alpha particle D) a beta particle 3. What is the number of electrons in an atom that has 20 protons and 17 neutrons? A) 37 B) 20 C) 3 D) Which phrase describes an Al atom? A) a negatively charged nucleus, surrounded by negatively charged electrons B) a negatively charged nucleus, surrounded by positively charged electrons C) a positively charged nucleus, surrounded by negatively charged electrons D) a positively charged nucleus, surrounded by positively charged electrons 5. Which conclusion was drawn from the results of the gold foil experiment? A) An atom is electrically neutral. B) An atom is mostly empty space. C) The nucleus of an atom is negatively charged. D) The electrons in an atom are located in specific shells. 6. Given the particle diagram: Which substance at STP can be represented by this particle diagram? A) N2 B) H2 C) Mg D) Kr 7. All phosphorus atoms have the same A) atomic number B) mass number C) number of neutrons plus the number of electrons D) number of neutrons plus the number of protons 8. The atomic mass of an element is the weighted average of the atomic masses of A) the least abundant isotopes of the element B) the naturally occurring isotopes of the element C) the artificially produced isotopes of the element D) the natural and artificial isotopes of the element
2 9. The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of bromine. Which numerical setup can be used to calculate the atomic mass of the element bromine? A) (78.92 u)(50.69) + (80.92 u)(49.31) B) (78.92 u)(49.31) + (80.92 u)(50.69) C) (78.92 u)(0.5069) + (80.92 u)(0.4931) D) (78.92 u)(0.4931) + (80.92 u)(0.5069) 10. Which electron configuration represents the electrons of an atom of neon in an excited state? A) 2-7 B) 2-8 C) D) Which term is defined as the region in an atom where an electron is most likely to be located? A) nucleus B) orbital C) quanta D) spectra 12. Which atom in the ground state has the same electron configuration as a calcium ion, Ca 2+, in the ground state? A) Ar B) K C) Mg D) Ne
3 Base your answers to questions 13 and 14 on the information below and on your knowledge of Rubidium and iodine have different chemical and physical properties. Some of these properties are shown in the table below. 13. Compare the electrical conductivity of these two elements at STP. 14. State the chemical property of iodine listed in this table. Base your answers to questions 15 and 16 on the information below and on your knowledge of The bright-line spectra for four elements and a mixture of elements are shown in the diagram below. 15. Explain, in terms of electrons and energy states, how the light emitted by excited atoms is produced. 16. Write the letter of each element present in the mixture. 17. Compare the energy of an electron in the first shell of a cadmium atom to the energy of an electron in the third shell of the same atom. 18. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar.
4 Base your answers to questions 19 through 22 on the information below and on your knowledge of The radius of a lithium atom is 130 picometers, and the radius of a fluorine atom is 60 picometers. The radius of a lithium ion, Li +, is 59 picometers, and the radius of a fluoride ion, F, is 133 picometers. 19. Describe the general trend in atomic radius as each element in Period 2 is considered in order from left to right. 20. In the space provided, draw a Lewis electron-dot diagram for a fluoride ion. 21. Explain, in terms of subatomic particles, why the radius of a lithium ion is smaller than the radius of a lithium atom. 22. Compare the radius of a fluoride ion to the radius of a fluorine atom. 23. 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 24. Which list of elements consists of a metal, a metalloid, and a nonmetal? A) Li, Na, Rb B) Cr, Mo, W C) Sn, Si, C D) O, S, Te 25. Which property can be defined as the ability of a substance to be hammered into thin sheets? A) conductivity B) malleability C) melting point D) solubility
5 26. The chart below shows the crystal shapes and melting points of two forms of solid phosphorous. Which phrase describes the two forms of phosphorus? A) same crystal structure and same properties B) same crystal structure and different properties C) different crystal structure and different properties D) different crystal structure and same properties 27. Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr 28. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state? A) B) C) D) 29. An atom of which element has the strongest attraction for the electrons in a bond? A) aluminum B) carbon C) chlorine D) lithium 30. Which atom in the ground state requires the least amount of energy to remove its valence electron? A) lithium atom B) potassium atom C) rubidium atom D) sodium atom 31. Which substance can not be broken down by a chemical change? A) ammonia B) ethanol C) tungsten D) water
6 Base your answers to questions 32 through 35 on the information below and on your knowledge of The diagrams below represent four different atomic nuclei. 32. Identify the nucleus above that is found in an atom that has a stable valence electron configuration. 33. Explain why nucleus 2 and nucleus 4 represent the nuclei of two different isotopes of the same element. 34. Determine the mass number of the nuclide represented by nucleus Identify the element that has atomic nuclei represented by nucleus Base your answer to the following question on the information below and on your knowledge of There are six elements in Group 14 on the Periodic Table. One of these elements has the symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium. State the expected number of valence electrons in an atom of the element flerovium in the ground state.
Which order of statements represents the historical development of the atomic model? A) C D A B B) C D B A C) D B A C D) D B C A
1. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C) an alpha particle D) a beta particle 2. What is the number of electrons in an atom that has 20 protons and 17
Periodic 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
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.
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.
Unit 2: Atomic Structure Additional Practice
Name: Unit 2: Atomic Structure Additional Practice Period: 1. Which particles have approximately the same mass? an electron and an alpha particle an electron and a proton a neutron and an alpha particle
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
Name: Teacher: Gerraputa
Name: Teacher: Gerraputa 1. Which list of elements contains a metal, a metalloid, and a nonmetal? 1. Ag, Si, I 2 3.K, Cu, Br 2 2. Ge, As, Ne 4.S, Cl 2, Ar 2. The elements on the Periodic Table are arranged
2015 Name: Test 1 Atomic Structure
2015 Name: Test 1 Atomic Structure 1. During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms A) return to lower energy
Regents 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
Practice 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
Name: 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
11. 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
A) 12 u C) K, Ca, Sc C) An electron has a negative charge and is located outside the nucleus. C) number of valence electrons
1. An atom that contains six protons, six neutrons, and six electrons has a mass of approximately A) 12 u B) 12 g C) 18 u D) 18 g 2. What is the correct Lewis electron-dot structure for the compound magnesium
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
Atomic Structure Practice Questions
Atomic Structure Practice Questions 1. Experiments performed to reveal the structure of atoms led scientists to conclude that an atom s (1) positive charge is evenly distributed throughout its volume (2)
Exam 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
Periodic 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
4. The mass of a proton is approximately equal to the mass of A an alpha particle C a positron. B a beta particle D a neutron
1. Which particles have approximately the same mass? A an electron and an alpha particle B an electron and a proton C a neutron and an alpha particle D a neutron and a proton 2. Which phrase describes
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
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
Chapter 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
Collegiate Institute for Math and Science Day 57: December 9, 2016 Room 427
Unit 2: Atomic Concepts Outline Name: Period: Date: 1. The modern model of the atom has evolved over a long period of time through the work of many scientists. Dalton s Model: Elements are made of atoms
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 are metals. 3. Which element is
Unit 2 Exam: Atomic Structure
Name: Unit 2 Exam: Atomic Structure Date: 1. What is the total number of valence electrons in an atom of germanium in the ground state? A) 8 B) 2 C) 14 D) 4 2. An electron has a charge of A) 1 and the
atomic structure practice test D) neutrons and protons B) empty space and has a small, positively charged nucleus C) neutron
atomic structure practice test 1. The major portion of an atom's mass consists of A) electrons and protons B) electrons and neutrons C) neutrons and positrons D) neutrons and protons 2. Which subatomic
Name: Date: Atomic Structure 2017 Mrs. Mannion Version 1
Name: Atomic Structure 2017 1. The mass of a proton is approximately equal to the mass of A) a beta particle B) an electron C) an alpha particle D) a neutron 2. What are the characteristics of a neutron?
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
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
Teacher: 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
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:
Work hard. Be nice. Name: Period: Date: UNIT 3: Electrons Lesson 4: The Octet Rule. Nitrogen Neon Carbon He
Name: Period: Date: UNIT 3: Electrons Lesson 4: The Octet Rule Do Now: By the end of today, you will have an answer to: What role do valence electrons play in chemical changes? Draw the following lewis
Unit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016
Name: PRACTICE QUESTIONS Date: 2/23/2016 1. Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of
Bonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
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.
Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
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
Unit 3 Atomics Repair Problems
1. What is the charge of the nucleus in an atom of oxygen-17? A) 0 B) 2 C) +8 D) +17 2. A neutral atom contains 12 neutrons and 11 electrons. The number of protons in this atom is A) 1 B) 11 C) 12 D) 23
Atomic Concepts and Nuclear Chemistry Regents Review
1. In the late 1800s, experiments using cathode ray tubes led to the discovery of the 10.Compared to an atom of phosphorus-31, an atom of sulfur-32 contains A) electron B) neutron C) positron D) proton
MULTIPLE 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.
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,
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
3.1 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
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.
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,
"In Terms Of" 1. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar.
Name: Mrs. Vandergoot "In Terms Of" Regents Chemistry 1. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar. 2. Base your answer to the following question on the
Name: Period: Date: Find the following elements according to their group and period: Write the excited state electron configuration of Na.
Name: Period: Date: UNIT 3: Electrons Lesson 3: Small particles, big similarities Do Now: By the end of today, you will have an answer to: Why do elements within the same group react similarly? Find the
Test 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
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
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
Regents Chemistry PRACTICE PACKET. Unit 2: Atomic Theory
*STUDENT* *STUDENT* Regents Chemistry PRACTICE PACKET Unit 2: Atomic Theory 2 Copyright 2015 Tim Dolgos Name History of Atomic Theory Period Fill in the missing information in the chart below: Name of
D) g. 2. In which pair do the particles have approximately the same mass?
1. A student constructs a model for comparing the masses of subatomic particles. The student selects a small, metal sphere with a mass of gram to represent an electron. A sphere with which mass would be
A) first electron shell D) are located in orbitals outside the nucleus A) 2-3 D) 18 A) K and Na C) a mixture C) Sb2O5
1. In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the A) first electron shell B) second electron shell C) third electron shell D) fourth electron
Question #1: Wednesday January AGENDA YOYO Practice Test Review. AIM Midterm Review
Wednesday January 15 2019 AIM Midterm Review YOYO Take YOYO sheet and start working on it Take out practice test and note the questions you want to go over today AGENDA YOYO Practice Test Review HOMEWORK
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations. Station Review Midterm January 2014 STATION 1: Chemical/physical properties and change
Name: Date: STATION 1: Chemical/physical properties and change Physical changes are changes in matter in which the appearance of a substance changes but the identity of the compound remains the same Chemical
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
Atomic Model and Periodic Table Test Review
Atomic Model and Periodic Table Test Review A. Give the family name for each description. 1. I have 1 electron on my outer shell. 2. One of the elements has 35 protons. 3. I have 2 electrons on my outer
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
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
Practice Packet Unit 4: Atomic Structure
Name: Regents Chemistry Practice Packet Unit 4: Atomic Structure Assess Yourself: Vocab: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson 7: 1 Vocabulary: Check your understanding. Describe
A) neutron C) Magnesium reacts with an acid. C) gamma radiation D) a proton
1. Which statement describes a chemical property of the element magnesium? A) Magnesium is malleable. B) Magnesium conducts electricity. C) Magnesium reacts with an acid. D) Magnesium has a high boiling
2. Atoms with nearly empty valence shells give up electrons. They are called
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations 4.8 Ions and Ionic Radius Directions: As we watch the video, answer these questions. 1. What is it called when an atom gains or loses an electron?
14: BEHOLD THE POWER OF THE NUCLEUS!!!
Name: Period: Date: UNIT 14: Nuclear Chemistry Lesson 1: Let s go nuclear! By the end of today, you will have an answer to: What does it mean to be radioactive? Do Now: Final problems related to electrochemistry
Test Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
2) Complete the following table. Take into account that all the atoms in it are neutral atoms: Copper Uranium Phosphorus 15 16
1) Describe Thomson's atomic model and draw it. THOMSON (1897): an atom is a solid sphere positively charged matter with embedded. 2) Complete the following table. Take into account that all the atoms
Textbook: Section B, Chapter 1
Atoms and the Periodic Table Review Sheet Textbook: Section B, Chapter 1 1. What is the Atomic number of nitrogen? 2. How many protons does nitrogen have? 3. How many electrons does nitrogen have? 4. How
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
Atomic Structure. 1. Write one electron configuration for an atom of silicon in an excited state.
tomic Structure Name: ate: 1. Write one electron configuration for an atom of silicon in an excited state. 5. Which electron configuration represents an atom of chlorine in an excited state?. 2 8 7. 2
Biotech 2: Atoms and Molecules OS Text Reading pp Electron cloud Atoms & Nucleus 2e Subatomic Particles Helium Electron cloud
9/4/017 Biotech : Atoms and Molecules OS Text Reading pp. 34-4 Atoms & Subatomic Particles Nucleus Helium e cloud cloud e Protons Neutrons Mass number = 4 s Nucleus Carbon atomic number = # of protons
THE PERIODIC TABLE, OBSERVABLE PROPERTIES & ATOMIC THEORY
CH 11 T7 THE PERIODIC TABLE & ATOMIC THEORY 1 You have mastered this topic when you can: 1) relate stability of the NOBLE GASSES to electron arrangement within the atom. 2) relate the charge of MONATOMIC
Chapter 2: Atoms. 2.1 (a) NaClO 3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222.
2.1 (a) NaClO 3 (b) AlF 3 2.2 (a) The mass number is 15 + 16 = 31. (b) The mass number is 86 + 136 = 222. 2.3 (a) The element has 15 protons, making it phosphorus (P); its symbol is 31 P 15. (b) The element
1. Demonstrate knowledge of the three subatomic particles, their properties, and their location within the atom.
1. Demonstrate knowledge of the three subatomic particles, their properties, and their location within the atom. 2. Define and give examples of ionic bonding (e.g., metal and non metal) and covalent bonding
E J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
Chemistry. The building blocks of matter Made of protons, neutrons and electrons. Pure substances that cannot be separated.
Chemistry CHEMISTRY NOTES Atom- Element- Compound- Molecule- The building blocks of matter Made of protons, neutrons and electrons. Pure substances that cannot be separated. Ex: Gold 2 or more elements
Practice Packet Unit: 5 Periodic Table
Regents Chemistry: Practice Packet Unit: 5 Periodic Table 1 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help
Name 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
Electronic 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
Ionic 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
Chapter 2: Atoms. 2.1 (a) NaClO3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222.
2.1 (a) NaClO3 (b) AlF3 2.2 (a) The mass number is 15 + 16 = 31. (b) The mass number is 86 + 136 = 222. 2.3 (a) The element has 15 protons, making it phosphorus (P); its symbol is 31 P 15. (b) The element
Chapter 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:
Regular Chemistry - 1st Semester Final Practice Exam
Regular Chemistry - 1st Semester Final Practice Exam Mr. Matthew Totaro MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement about the
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
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.
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
Chemistry 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
A. Cu 2+ B. Fe 2+ C. Ca 2+ D. Hg Which atom in the ground state has three halffilled orbitals?
Unit 3 - Electrons, Light, and Ions 15-16 Name: ate: 1. Which is the electron configuration of a neutral atom in the ground state with a total of six valence electrons?. 1s 2 2s 2 2p 2. 1s 2 2s 2 2p 4.
End of Semester 1 Review
Name: ate: 1. In the modern Periodic Table, the elements are arranged in order of increasing. atomic number. mass number. oxidation number. valence number 5. Which element within any given period of the
THE PERIODIC TABLE, OBSERVABLE PROPERTIES & ATOMIC THEORY
CH 11 T7 THE PERIODIC TABLE & ATOMIC THEORY 1 You have mastered this topic when you can: 1) relate stability of the NOBLE GASSES to electron arrangement within the atom. 2) relate the charge of MONATOMIC
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (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
Note Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by
Note Taking Guide: Episode 401 Dmitri Mendeleev: arranged elements by. predicted of missing. Henry Moseley: discovered that each has a unique. arranged elements by. now all elements fit into place based
What is the smallest particle of the element gold (Au) that can still be classified as gold? A. atom B. molecule C. neutron D.
Use the Periodic Table of Elements to answer the following question(s). Which sentence about the periodic table of elements is true? A. All elements in period 2 are metals. B. All elements in group 18
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law
A. They are noble (inert) gases. B. They are nonmetals. C. They have the same thermal conductivity. D. They have the same number of protons.
toms, Elements, ompounds and Mixtures Name: 1. Which statement is true about the charges assigned to an electron and a proton?. oth an electron and a proton are positive.. n electron is positive and a
Chapter 5 Review/Practice Test
Chapter 5 Review/Practice Test Name Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Electrons involved in bonding between atoms are a. closest to the nucleus.
Chapter 4 Atoms and Elements
Atoms and Elements Experiencing Atoms Atoms are incredibly small, yet they compose everything. Atoms are the pieces of elements. Properties of the atoms determine the properties of the elements. 2 The
Chemistry Common 2. A. Na B. Mg C. Ne D. Ag. 2. In the modern Periodic Table, the elements are arranged in order of increasing
hemistry ommon 2 Name: ate: 1. Which symbol represents an alkaline earth element? 1.. Na. Mg. Ne. g 2. In the modern Periodic Table, the elements are arranged in order of increasing 2.. atomic number.
Name: 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.
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
Practice Packet Level 3: Atomics
Name: Regents Chemistry: Mr. Palermo Practice Packet Level 3: Atomics Name: Unit Vocabulary: For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions.
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)
Trends of the Periodic Table Notes
Trends of the Periodic Table Notes 1. A salute to who invented the modern Table. 2. There are trends that go up and down in on the table. 3. There are other trends that go left and right in on the table.