Mid-Term Review Multiple Choice: Ch. 3 Identify the letter of the choice that best completes the statement or answers the question.

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1 HONORS CHEMISTRY MID-TERM PRACTICE January 2013 Mrs. Allen from HS North put together a collection of multiple choice questions for you to use as a study tool. Not all of the midterm topics are covered here, however make sure you reference the topic list as you prepare for the test!! And review your old tests from this year as well. Mid-Term Review Multiple Choice: Ch. 3 Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following measurements is expressed to three significant figures? a m c km b mg d mm 2. In the measurement L, which digit is the estimated digit? a. 5 b. the 0 immediately to the left of the 3 c. 3 d. the 0 to the left of the decimal point 3. How many significant figures are in the measurement grams? a. two c. four b. three d. five 4. What is the volume of a salt crystal measuring m by m by m? a m 3 c m 3 b m 3 d m 3 5. What quantity is represented by the metric system prefix deci-? a c. 0.1 b. 100 d Which temperature scale has no negative temperatures? a. Celsius c. Joule b. Fahrenheit d. Kelvin Commonly Used Metric Prefixes Prefix Meaning Factor mega (M) 1 million times larger than the unit it precedes 10 kilo (k) 1000 times larger than the unit it precedes 10 deci (d) 10 times smaller than the unit it precedes 10 centi (c) 100 times smaller than the unit it precedes 10 milli (m) 1000 times smaller than the unit it precedes 10 micro ( ) 1 million times smaller than the unit it precedes 10 nano (n) 1000 million times smaller than the unit it precedes 10 pico (p) 1 trillion times smaller than the unit it precedes 10 Honors Chemistry Mid-Term Review Page 1

2 7. What is the quantity meters expressed in centimeters? Use the table above to help you. a cm c. 7.5 cm b cm d cm 8. Which of the following equalities is NOT correct? Use the table above to help you. a. 100 cg = 1 g c. 1 cm 3 = 1 ml b mm = 1 m d. 10 kg = 1 g 9. Density is found by dividing. a. mass by volume c. mass by area b. volume by mass d. area by mass 10. If a liter of water is heated from 20 C to 50 C, what happens to its volume? a. The volume decreases. b. The volume increases. c. The volume first increases, then decreases. d. The volume first decreases, then increases. Answer Section 1. ANS: C 2. ANS:C 3. ANS: D 4. ANS:C 5. ANS: C 6. ANS:D 7. ANS: B 8. ANS:D 9.ANS: A 10. ANS: B Multiple Choice: Ch. 2 Identify the letter of the choice that best completes the statement or answers the question. 1. A golf ball has more mass than a tennis ball because it. a. takes up more space c. contains different kinds of matter b. contains more matter d. has a definite composition 2. All of the following are physical properties of matter EXCEPT. a. mass c. melting point b. color d. ability to rust 3. Which of the following is NOT a physical property of water? a. It has a boiling point of 100 C. b. It is a colorless liquid. c. It is composed of hydrogen and oxygen. d. Sugar dissolves in it. 4. Which of the following are considered physical properties of a substance? a. color and odor c. malleability and hardness b. melting and boiling points d. all of the above 5. Which of the following materials is a substance? a. air c. stainless steel b. gasoline d. silver 6. Which of the following is used for chemical symbols today? a. drawings c. letters b. icons d. numbers 7. The chemical formula of a compound does NOT indicate the. a. identity of the elements in the compound b. how elements are joined in the compound c. the composition of the compound Honors Chemistry Mid-Term Review Page 2

3 d. relative proportions of the elements in the compound 8. In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the following is a reactant? a. sucrose c. water b. carbon dioxide d. heat 9. Which of the following indicates that a chemical change has happened during cooking? a. The food darkens. b. Bubbles form in boiling water. c. Butter melts. d. Energy is transferred from the stove to a pan. 10. Which action changes the identity of the substance referenced? a. melting gold b. running an electric current through copper c. corroding iron d. breaking an ice cube Answer Section 1. ANS: B 2. ANS: D 3. ANS: C 4. ANS: D 5. ANS: D 6. ANS: C 7. ANS: B 8. ANS: A 9. ANS: A 10. ANS: C Multiple Choice: Ch. 4 Identify the letter of the choice that best completes the statement or answers the question. 1. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements? a. Cathode rays are negatively-charged particles. b. Cathode rays can be deflected by magnets. c. An electron is 2000 times lighter than a hydrogen atom. d. Charge-to-mass ratio of electrons was the same, regardless of the gas used. 2. Which of the following is true about subatomic particles? a. Electrons are negatively charged and are the heaviest subatomic particle. b. Protons are positively charged and the lightest subatomic particle. c. Neutrons have no charge and are the lightest subatomic particle. d. The mass of a neutron nearly equals the mass of a proton. 3. Which of the following is correct concerning subatomic particles? a. The electron was discovered by Goldstein in b. The neutron was discovered by Chadwick in c. The proton was discovered by Thomson in d. Cathode rays were found to be made of protons. 4. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true? a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom. b. The nucleus is made of protons, electrons, and neutrons. c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom. d. The nucleus is made of electrons and protons. 5. What does the number 84 in the name krypton-84 represent? a. the atomic number c. the sum of the protons and electrons Honors Chemistry Mid-Term Review Page 3

4 b. the mass number d. twice the number of protons 6. Isotopes of the same element have different. a. numbers of neutrons c. numbers of electrons b. numbers of protons d. atomic numbers 7. In which of the following is the number of neutrons correctly represented? a. F has 0 neutrons. c. Mg has 24 neutrons. b. As has 108 neutrons. d. U has 146 neutrons. 8. Which of the following isotopes has the same number of neutrons as phosphorus-31? a. P c. Si b. S 9. The atomic mass of an element depends upon the. a. mass of each electron in that element b. mass of each isotope of that element c. relative abundance of protons in that element d. mass and relative abundance of each isotope of that element d. Si Answer Section 1. ANS: D 2. ANS:D 3. ANS: B 4. ANS: C 5. ANS: B 6. ANS: A 7. ANS: D 8. ANS: B 9. ANS: D Multiple Choice: Ch. 25 Identify the letter of the choice that best completes the statement or answers the question. 1. A beta particle is a(n). a. photon c. helium nucleus b. electron d. hydrogen nucleus 2. What is the change in the atomic number when an atom emits an alpha particle? a. decreases by 2 c. increases by 1 b. decreases by 1 d. increases by 3. What is the change in atomic number caused by the emission of gamma radiation? a. decreases by 2 c. remains the same b. decreases by 1 d. increases by 1 4. Which symbol is used for an alpha particle? a. He b. He c. d. He He 5. What particle decomposes to produce the electron of beta radiation? a. proton c. electron b. neutron d. positron 6. What symbol is used for beta radiation? a. e c. e Honors Chemistry Mid-Term Review Page 4

5 b. e d. e 7. If an isotope decays by the process of beta emission,. a. the mass number changes b. the atomic number changes c. protons are given off d. the number of neutrons remains the same Answer Section 1. ANS: B 2. ANS:A 3. ANS: C 4. ANS:D 5. ANS: B 6. ANS:B 7. ANS: B Multiple Choice: Ch. 5 and Ch. 6 Identify the letter of the choice that best completes the statement or answers the question. 1. How many energy sublevels are in the second principal energy level? a. 1 c. 3 b. 2 d When an electron moves from a lower to a higher energy level, the electron. a. always doubles its energy b. absorbs a continuously variable amount of energy c. absorbs a quantum of energy d. moves closer to the nucleus 3. What is the number of electrons in the outermost energy level of an oxygen atom? a. 2 c. 6 b. 4 d Which electron configuration of the 4f energy sublevel is the most stable? a. 4f c. 4f b. 4f d. 4f 5. Which of the following electron configurations of outer sublevels is the most stable? a. 4d 5s c. 4d 5s b. 4d 5s d. 4d 5s 6. Which variable is directly proportional to frequency? a. wavelength c. position b. velocity d. energy 7. How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom? a. They are greater in magnitude than those between lower energy levels. b. They are smaller in magnitude than those between lower energy levels. c. There is no significant difference in the magnitudes of these differences. d. No answer can be determined from the information given. 8. Bohr's model could only explain the spectra of which type of atoms? a. single atoms with one electron b. bonded atoms with one electron c. single atoms with more than one electron d. bonded atoms with more than one electron 9. The wavelike properties of electrons are useful in. a. defining photons b. writing electron configurations c. magnifying objects d. determining the velocity and position of a particle 10. Which of the following categories includes the majority of the elements? Honors Chemistry Mid-Term Review Page 5

6 a. metalloids c. metals b. liquids d. nonmetals 11. Which of the following groupings contains only representative elements? a. Cu, Co, Cd c. Al, Mg, Li b. Ni, Fe, Zn d. Hg, Cr, Ag 12. Which of the following is true about the electron configurations of the representative elements? a. The highest occupied s and p sublevels are completely filled. b. The highest occupied s and p sublevels are partially filled. c. The electrons with the highest energy are in a d sublevel. d. The electrons with the highest energy are in an f sublevel. 13. What causes the shielding effect to remain constant across a period? a. Electrons are added to the same principal energy level. b. Electrons are added to different principal energy levels. c. The charge on the nucleus is constant. d. The atomic radius increases. 14. Atomic size generally. a. increases as you move from left to right across a period b. decreases as you move from top to bottom within a group c. remains constant within a period d. decreases as you move from left to right across a period 15. Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases? a. more shielding of the electrons by the highest occupied energy level b. an increase in size of the nucleus c. an increase in number of protons d. fewer electrons in the highest occupied energy level 16. In which of the following sets are the charges given correctly for all the ions? a. Na, Mg, Al c. Rb, Ba, P b. K, Sr, O d. N, O, F 17. In which of the following groups of ions are the charges all shown correctly? a. Li, O, S c. K, F, Mg b. Ca, Al, Br d. Na, I, Rb 18. For Group 2A metals, which electron is the most difficult to remove? a. the first b. the second c. the third d. All the electrons are equally difficult to remove. 19. Of the following elements, which one has the smallest first ionization energy? a. boron c. aluminum b. carbon d. silicon Answer Section 1. ANS: B 2. ANS:C 3. ANS: C 4. ANS:D 5. ANS: A 6. ANS:D 7. ANS: B 8. ANS:A 9. ANS: C 10. ANS:C 11. ANS: C 12. ANS:B 13. ANS: A 14. ANS:D 15. ANS: A 16. ANS:B 17. ANS: B 18. ANS:C 19. ANS: C Multiple Choice: Ch. 7 & 8 Honors Chemistry Mid-Term Review Page 6

7 Identify the letter of the choice that best completes the statement or answers the question. 1. How does calcium obey the octet rule when reacting to form compounds? a. It gains electrons. b. It gives up electrons. c. It does not change its number of electrons. d. Calcium does not obey the octet rule. 2. What is the electron configuration of the oxide ion (O -2 )? a. 1s 2 2s 2 2p 2 c. 1s 2 2s 2 b. 1s 2 2s 2 2p 6 d. 1s 2 2s 2 2p 4 3. What is the electron configuration of the iodide ion? a. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 1 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4. What is the net charge of the ionic compound calcium fluoride? a. 2 c. 0 b. 1 d What is the formula unit of aluminum oxide? a. AlO c. AlO b. Al O d. Al O 6. What is the name of the ionic compound formed from lithium and bromine? a. lithium bromine c. lithium bromium b. lithium bromide d. lithium bromate 7. What is the formula for sodium sulfate? a. NaSO c. Na(SO ) b. Na SO d. Na (SO ) 8. What does the term coordination number in ionic crystals refer to? a. the total number of valence electrons in an atom b. the number of oppositely charged ions surrounding a particular ion c. the number of atoms in a particular formula unit d. the number of like-charged ions surrounding a particular ion 9. Under what conditions can potassium bromide conduct electricity? a. only when melted b. only when dissolved c. only when it is in crystal form d. only when melted or dissolved in water 10. Which of the following elements can form diatomic molecules held together by triple covalent bonds? a. carbon c. fluorine b. oxygen d. nitrogen 11. Which elements can form diatomic molecules joined by a single covalent bond? a. hydrogen only b. halogens only c. halogens and members of the oxygen group only d. hydrogen and the halogens only 12. Which of the following electron configurations gives the correct arrangement of the four valence electrons of the carbon atom in the molecule methane (CH )? a. 2s 2 2p 2 c. 2s 1 2p 2 3s 2 b. 2s 1 2p 1 3s 1 d. 2s 1 2p Which of the following diatomic molecules is joined by a double covalent bond? a. c. b. d. Honors Chemistry Mid-Term Review Page 7

8 14. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible? a. pairs of valence electrons c. mobile electrons b. inner shell electrons d. the electrons closest to the nuclei 15. What causes water molecules to have a bent shape, according to VSEPR theory? a. repulsive forces between unshared pairs of electrons b. interaction between the fixed orbitals of the unshared pairs of oxygen c. ionic attraction and repulsion d. the unusual location of the free electrons 16. Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen? a. C c. O b. Na d. S Answer Section 1. ANS: B 2. ANS: B 3. ANS: A 4. ANS: C 5. ANS: D 6. ANS: B 7. ANS: B 8. ANS: B 9. ANS: D 10. ANS: D 11. ANS: D 12. ANS: D 13. ANS: A 14. ANS: A 15. ANS: A 16. ANS: C Honors Chemistry Mid-Term Review Page 8

Bonding 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