Name
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Class
Date
Organization of Matter
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Test
Unit
2
DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that best
completes the statement.
1. Which of the following points is NOT a part of Dalton's atomic theory? (a) atoms cannot be
subdivided or created (b) the number of protons in an atom is the atomic number
(c) in chemical reactions, atoms are combined, separated, or rearranged (d) all matter is
composed of extremely small particles called atoms
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2. Since Dalton's atomic theory stated that atoms could not be destroyed, the theory supported
the (a) law of conservation of mass; (b) law of conservation of energy; (c) law of combining
ratios; (d) concept of isotopes.
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3. If two or more compounds are composed of the same two elements, the masses of the second
element combined with a fixed mass of the first element to make the compounds can be
expressed as simple whole-number ratios. This is a statement of the law of (a) conservation of
mass; (b) mass action; (c) multiple proportions; (d) definite composition.
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4. Experiments with cathode rays led to the discovery of the (a) proton; (b) nucleus; (c) neutron;
(d) electron.
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5. Rutherford's work, which led to the discovery of the nucleus, involved experiments in which
positively-charged particles were (a) passed through a tube containing gas; (b) used to
bombard a cathode plate; (c) collided with electrons; (d) used to bombard thin, metal foil.
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6. The nucleus of most atoms is composed of (a) tightly packed protons; (b) tightly packed
neutrons; (c) tightly packed protons and neutrons; (d) loosely connected protons and
electrons.
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7. Atoms of the same element that have different masses are called (a) moles; (b) isotopes;
(c) ions; (d) neutrons.
8. A neutral carbon atom (atomic number 6) has (a) 3 electrons and 3 neutrons; (b) 6 protons;
(c) 3 protons and 3 electrons; (d) 3 protons and 3 neutrons.
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9. The atomic mass of a particular isotope is a(n) (a) average atomic mass; (b) isotopic mass
number; (c) atomic number; (d) relative atomic mass.
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10. The particle model of light explained the inability of certain kinds of light to remove electrons
from metals by stating that the light's (a) mass was too low; (b) frequency was too high;
(c) energy was too low; (d) wavelength was too short.
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11. The velocity of any type of electromagnetic radiation is equal to the product of the radiation's
wavelength and (a) mass; (b) color; (c) speed; (d) frequency.
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12. Since excited hydrogen atoms produce a specific line emission spectrum, scientists concluded
that hydrogen (a) had no electrons; (b) did not release photons; (c) released photons of only
certain energies; (d) could only exist in the ground state.
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13. The idea of orbitals of the quantum model of the atom resulted from descriptions of electrons
as (a) particles; (b) waves; (c) photons; (d) quanta.
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14. Quantum numbers are sets of numbers that specify the properties of (a) molecules;
(b) electrons; (c) ions; (d) gases.
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Unit 2
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15. The total number of orbitals that can exist at the second main energy level is (a) 2; (b) 3; (c) 4;
(d) 8.
16. If the third main energy level contains 15 electrons, how many more could it possibly hold?
(a) 0 (b) 1 (c) 3 (d) 17
17. Which of the following rules requires that each of the p orbitals at a particular level receives
one electron before any of them can have two electrons? (a) Hund's rule (b) the Pauli exclusion
principle (c) the Aufbau principle (d) the quantum rule
Organization of Matter
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18. The electron-dot notation for fluorine, atomic number 9, would show (a) 9 dots around the
symbol; (b) 1 dot next to the symbol; (c) 7 dots around the symbol; (d) 8 dots around the
symbol.
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19. With some exceptions, the elements in Mendeleev's periodic table were arranged in order of
increasing (a) atomic number; (b) density; (c) atomic mass; (d) reactivity.
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20. The periodic law allows the general properties of an element to be known based on the
element's (a) position in the Periodic Table; (c) number of isotopes; (c) symbol; (d) color.
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21. Evidence gathered after Mendeleev's time indicates that a better arrangement for elements in the ~
periodic table is by (a) mass number; (b) atomic number; (c) group number; (d) series number.
22. Calcium, atomic number 20, has the electron configuration [Ar] 4sz. What period is calcium
in? (a) 2 (b) 4 (c) 8 (d) 20
23. The group of 14 elements in the sixth period which are characterized by filling electrons in the
4f orbitals are known as (a) actinides; (b) lanthanides; (c) transition elements; (d) metalloids.
24. An unknown element is found to have the electron configuration [Kr] 4d5SsZ•
does this element belong? (a) 4 (b) S (c) 7 (d) 9
To what group
25. A measure of the power of an atom in a chemical compound to attract electrons is called
(a) electron affinity; (b) electron configuration; (c) e1ectronegativity; (d) ionization potential.
26. Comparison of the atomic radii of elements across a period would 'show a trend of
(a) gradual decrease; (b) gradual decrease, followed by sharp increase; (c) gradual increase;
(d) gradual increase, followed by sharp decrease.
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27. The number of valence electrons in Group 1 elements is (a) 1; (b) 2; (c) 8; (d) equal to the
period number.
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28. The electrostatic attraction between positively-charged nuclei and negatiyely-charged electrons
permits two atoms to be held together by a(n) (a) chemical bond; (b) London force;
(c) neutron; (d) ion.
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29. A chemical bond resulting from the sharing of electrons between two atoms is called a(n)
(a) ionic bond; (b) orbital bond; (c) Lewis structure; (d) covalent bond.
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30. If the electrons in a bond are shared equally between two atoms, the bond is (a) polar
covalent; (b) nonpolar covalent; (c) metallic; (d) ionic.
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31. The energy of two moles of uncombined hydrogen atoms compared to that of one mole of
Hz molecules is (a) equal; (b) always greater; (c) always less; (d) always half.
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32. The octet rule states that chemical compounds tend to form so that each atom has an octet of
electrons in (a) its highest occupied energy level; (b) the Is orbital; (c) its d orbitals; (d) its p
orbitals.
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33. After drawing the electron-dot symbols for each atom in a Lewis structure, one should
(a) determine the number of each type of atom in the molecule; (b) add unshared pairs of
electrons around nonmetal atoms; (c) determine the total number of valence electrons in each
atom; (d) determine the electronegativity of each atom.
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34. A charged group of covalently-bonded atoms is called a(n) (a) dipole; (b) double bond;
(c) polyatomic ion; (d) Lewis structure.
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36. A formula unit indicates the simplest unit of only a(n) (a) polar covalent compound;
(b) molecular compound; (c) any compound; (d) nonpolar covalent compound.
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37. Lattice energy is the energy released in the formation of a(n) (a) Lewis structure; (b) polar
covalent compound; (c) nonpolar covalent compound; (d) ionic compound.
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38. The orbitals that are vacant in the highest energy level of all the s -block metals are the
(a) p orbitals; (b) d orbitals; (c) s orbitals; (d) f orbitals.
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39. The model for predicting molecular geometry that is based on the assumption that electrons in
molecules repel each other is called (a) hybridization; (b) Lewis structure; (b) London force
model; (d) VSEPR theory.
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40. Use VSEPR theory to predict the shape of hydrogen chloride, HC!. (a) tetrahedral (b) linear
(c) bent (d) triangular planar
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35. How many electrons must be used in the Lewis structure of the hydroxide ion, OW?
(a) 1 (b) 8 (c) 9 (d) 10
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Unit 2
Organization of Matter
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