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2nd Quarter Exam _ Chemistry 1
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. The modern periodic table is arranged in order of increasing atomic ____.
a. radius
c. mass
b. number
d. charge
____
2. Which state of matter is characterized by having a definite volume but NO definite shape?
a. gas
c. solid
b. liquid
d. none of the above
____
3. Going down a group in the periodic table, electron shielding generally causes the effective nuclear charge to
a. vary unpredictably.
c. remain the same.
b. increase.
d. decrease.
____
4. Which of the following is true about subatomic particles?
a. Neutrons have no charge and are the lightest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. The mass of a neutron nearly equals the mass of a proton.
d. Electrons are negatively charged and are the heaviest subatomic particle.
____
5. The nonmetals in Groups 5A through7A ____.
a. have a numerical charge that is found by subtracting 8 from the group number
b. end in -ate
c. lose electrons when they form ions
d. all have ions with a –1 charge
____
6. Select the correct formula for sulfur hexafluoride.
a. F SO
c. S F
b. F S
d. SF
____
7. How do atoms achieve noble-gas electron configurations in single covalent bonds?
a. Two atoms share two pairs of electrons.
b. Two atoms share one electron.
c. Two atoms share two electrons.
d. One atom completely loses two electrons to the other atom in the bond.
____
8. The particles that are found in the nucleus of an atom are ____.
a. electrons only
c. neutrons and electrons
b. protons and neutrons
d. protons and electrons
____
9. Which of the following is an example of an extensive property of the metal, Nickel (Ni)?
a. mass of one sample of Nickel is 5g
c. boiling point is 1453 °C
b. color is silvery white
d. melting point is 2732 °C
____ 10. According to Dalton’s atomic theory, atoms
a. can be divided.
b. of different elements cannot combine.
c. are destroyed in chemical reactions.
d. of each element are identical in size, mass, and other properties.
____ 11. Which of the following elements has the lowest electronegativity?
a. lithium
c. carbon
b. bromine
d. fluorine
____ 12. An element that has an electron configuration of [Xe]2s22p3 is in Period _____ of the periodic table.
a. 4
c. 2
b. 1
d. 3
____ 13. Name the compound Zn3(PO4)2.
a. zinc potassium oxide
b. zinc phosphate
c. zinc phosphite
d. trizinc polyoxide
____ 14. Which of the following correctly provides the names and formulas of polyatomic ions?
a. sulfite: S ; sulfate: SO
b. carbonate: HCO ; bicarbonate: CO
c. nitrite: NO ; nitrate: NO
d. OH : hydroxide; O : oxide
____ 15. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. silver
c. silicon
b. selenium
d. nitrogen
____ 16. Under ordinary conditions, the particles in a gas are
a. held in fixed positions.
c. very far from each other.
b. unevenly distributed.
d. closely packed.
____ 17. Which of the following represents the noble-gas electron configuration for the element, yttrium (Y)? Show
the work for the regular electron configuation and noble gas configuration for Yttrium.
a. [Kr] 4d25s2
c. [Kr] 4d55s1
4 1
b. [Kr] 4d 5s
d. [Kr] 4d15s2
____ 18. Which of the following is a physical change?
a. rotting of food
b. evaporation
c. corrosion
d. explosion
____ 19. All of the following are examples of a chemical change EXCEPT ____.
a. milk souring
c. baking soda neutralizing stomach acid
b. snow melting
d. the explosion of dynamite
____ 20. The effect of inner electrons on the attraction between the nucleus and the outer electrons of an atom is called
a. electronegativity.
c. electron shielding.
b. electron ionization.
d. electron affinity.
____ 21. The elements in Group 7A are known by what name?
a. alkali metals
c. noble gases
b. alkaline-earth metals
d. halogens
____ 22. Using the periodic table, determine the number of neutrons in
the answer.
a. 11
c. 8
b. 12
d. 10
Mg. Show the work necessary for finding
____ 23. “Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and
all electrons in singly occupied orbitals must have the same spin” is a statement of
a. Hund’s rule.
c. the aufbau principle.
b. the quantum effect.
d. the Pauli exclusion principle.
____ 24. An element that has an electron configuration of [Ne]3s23p4 is in Group _____ of the periodic table.
a. 2
c. 6
b. 3
d. 5
____ 25. Which element, when combined with fluorine, would most likely form an ionic compound?
a. phosphorus
c. chlorine
b. carbon
d. lithium
____ 26. The statement that an electron occupies the lowest available energy orbital is
a. the aufbau principle.
c. Hund’s rule.
b. the Pauli exclusion principle.
d. Bohr’s law.
____ 27. Which of the following was NOT among Democritus’s ideas?
a. Matter consists of tiny particles called atoms.
b. Atoms retain their identity in a chemical reaction.
c. Atoms are indestructible.
d. Atoms are indivisible.
____ 28. What is one difference between a mixture and a compound?
a. A mixture must be uniform in composition.
b. A mixture can only be separated into its components by chemical means.
c. A compound consists of more than one phase.
d. A compound can only be separated into its components by chemical means.
____ 29. What is the formula unit of sodium nitride?
a. NaN
b. NaN
c. Na N
d. Na N
____ 30. The main energy levels of an atom are indicated by the
a. magnetic quantum numbers.
c. principal quantum numbers.
b. orbital quantum numbers.
d. spin quantum numbers.
____ 31. Atoms of the same element that have different masses are called
a. moles.
c. neutrons.
b. nuclides.
d. isotopes.
____ 32. Which is the best reason that the atomic radius generally increases with atomic number in each group of
elements?
a. A new octet forms.
b. The nuclear charge increases.
c. The number of neutrons increases.
d. The number of energy levels increases.
____ 33. Which scientist developed the quantum mechanical model of the atom?
a. Albert Einstein
c. Ernest Rutherford
b. Erwin Schrodinger
d. Niels Bohr
____ 34. In naming a binary molecular compound, the number of atoms of each element present in the molecule is
indicated by ____.
a. prefixes
c. Roman numerals
b. superscripts
d. suffixes
____ 35. Which of the following is a heterogeneous mixture?
a. milk
c. vinegar in water
b. air
d. oil and vinegar
____ 36. How many unpaired electrons are in a phosphorus atom (atomic number 15)? Show the work the for the
orbital notation (or arrow diagram) for this element. It should help you answer this question.
a. 1
c. 3
b. 2
d. 0
____ 37. Which of the following items is a mixture (NOT a compound)?
a. table salt
c. baking soda
b. table sugar
d. salad dressing
____ 38. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. neutral, with the number of protons equaling the number of electrons
c. negatively charged, with the number of electrons exceeding the number of protons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the
number of neutrons
____ 39. Which of the following statements is true about ions?
a. Cations form when an atom loses electrons.
b. Anions form when an atom loses protons.
c. Anions form when an atom gains protons.
d. Cations form when an atom gains electrons.
____ 40. The homogeneous mixture in the illustration above is in container
a. a.
c. c.
b. b.
d. d.
____ 41. Which of the following elements has the smallest ionic radius?
a. O
c. K
b. S
d. Li
____ 42. Which is a typical characteristic of an ionic compound?
a. The ionic compound is described as a molecule.
b. The ionic compound has a high melting point.
c. The ionic compound has a low solubility in water.
d. Electron pairs are shared among atoms.
____ 43. What is the electron configuration of the oxide ion (O )? Show the work the electron configuration of
the atom and the ion in this problem.
a. 1s 2s 2p
c. 1s 2s 2p
b. 1s 2s 2p
d. 1s 2s
____ 44. How many valence electrons does a helium atom have?
a. 3
c. 5
b. 4
d. 2
____ 45. Experiments with cathode rays led to the discovery of the
a. electron.
c. neutron.
b. proton.
d. nucleus.
____ 46. The quantum mechanical model of the atom ____.
a. has many analogies in the visible world
b. was proposed by Niels Bohr
c. involves the probability of finding an electron in a certain position
d. defines the exact path of an electron around the nucleus
____ 47. When the octet rule is satisfied, the outermost _____ are filled.
a. s and d orbitals
c. d and f orbitals
b. s and p orbitals
d. d and p orbitals
____ 48. Who explained the behavior of positively charged particles being deflected from a metal foil as the nucleus?
a. John Dalton
c. Ernest Rutherford
b. James Chadwick
d. Niels Bohr
____ 49. Which of the following diatomic molecules is joined by a double covalent bond?
a.
c.
b.
d.
____ 50. What is the formula unit of aluminum oxide?
a. Al O
b. Al O
c. AlO
d. AlO
____ 51. The sum of the protons and neutrons in an atom equals the ____.
a. average atomic mass
c. atomic number
b. mass number
d. nucleus number
____ 52. Who predicted that all matter can behave as waves as well as particles?
a. Louis de Broglie
c. Max Planck
b. Albert Einstein
d. Erwin Schrodinger
____ 53. Which of the following is the correct name for N O ?
a. nitrous oxide
c. nitrate oxide
b. nitrogen dioxide
d. dinitrogen pentoxide
____ 54. According to Bohr’s theory, an excited atom would
a. jump all over the place.
c. collapse.
b. absorb photons.
d. release energy in the form of light.
____ 55. Binary molecular compounds are made of two ____.
a. polyatomic ions
c. cations
b. metallic elements
d. nonmetallic elements