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Winter Homework
Multiple Choice:
1. When x-ray and infrared radiation are traveling in a vacuum, they have the same
1. speed
2. frequency
3. wavelength
4. energy per photon
2. The speed of an electromagnetic wave can be calculating
1. frequency + wavelength
2. frequency - wavelength
3. frequency x wavelength
4. frequency ÷ wavelength
3. A high frequency electromagnetic wave that has a shorter wavelength and higher
frequency than all other types of electromagnetic waves:
1. radio wave
2. microwave
3. ultraviolet wave
4. gamma ray
4. The electromagnetic spectrum is organized according to:
1. wave source 2. danger to humans 3. frequency and wavelength
5. Most of Earth's radiant energy comes from the
1. Earth,
2. Sun
3. Moon.
4. color
4. Atmosphere
6. The maximum amount of electrons that can fit inside of an s orbital:
1. 1
2. 2
3. 6
4. 10
7. The mathematical function that describes the behavior of electrons in an atom:
1. Atomic orbital 2. Aufbau principle 3. Bohr's model 4. Emission spectra
8. Which of the following compounds is a covalent compound?
1. LiCl
2. BaO
3. HI
4. CaS
9. When electrons in an atom receive energy from an outside source, the electron will
most likely
1. move to an excited state
2. move to the ground state
3. create a covalent bond
4. change into a proton
10. An atom with 17 electrons contains how many core and valence electrons:
1. 2 core and 15 valence
2. 8 core and 9 valence
3. 10 core and 7 valence
4. 15 core and 2 valence
11. Which of the following electron configurations represents the most stable
configuration?
1. 1s²2s²2p⁶
2. 1s²2s²2p⁵
3. 1s²2s²2p⁴
4. 1s²2s²2p³
12. What is a feature of elements that are found in the same group in the periodic table?
1. They have similar chemical properties 2. They have the same ionization energy
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3. They have similar atomic radii
4. There is no relationship
13. When moving left to right on the periodic table, ionization energy tends to:
1. increase
2. decrease
3. remain the same 4. there is no regular pattern
14. Ionization energies for element X (kJ/mol): 1815(2ⁿᵈ), 2740(3ʳᵈ), 11600(4ᵗʰ),
14800(5ᵗʰ).
Using the data shown, element X is most likely to be:
1. Na
2. Mg
3. Al
4. Si
15. Group 18 elements have ___ valence electrons.
1. 6(six)
2. 7(seven)
3. 8(eight)
4. 0(zero)
16. Which of the following atoms contains only three valence electrons?
1. Li
2. B
3. N
4. F
17. In terms of quantum numbers,what does 4d represent?
1. n = 4, L = 1 2. n = 4, L = 2 3. n = 2, L = 3 4. n = 3, L = 4
18. In an atom, which has the largest mass?
1. proton
2. neutron
3. electron
4. nucleus
19. Which of the following can be the quantum numbers for an orbital?
1. n = 4, l = 4, mₗ = 3 2. n = 2, l = 3, mₗ = 1 3. n = 3, l = 2, mₗ = -1 4. n = 3, l = 0, mₗ
= -3
20. The probability of finding an electron is the same in every direction from the nucleus in
which orbital?
1. s
2. p
3. d
4. f
21. The maximum number of electrons with l = 3 is
1. 2
2. 6
3. 10
4. 14
22. Which of the following would increase the kinetic energy of ejected electrons from a
metal surface?
1. increasing the brightness of the light
2. increasing the frequency of the light
3. increasing the wavelength of the light
4. none of the provided answers
23. When electrons are removed from an atom to form an ion, the atomic radius of that
atom will
1. increase
2. decrease
3. stay the same
4. unable to determine
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Winter Homework
24. Which group(g) of elements would be the most non-reactive?
1. Alkali metals(g1) 2. Alkaline earth metals(g2)
3. Halogens(g17)
4. Noble gases(g18)
25. Which group of elements would be the most reactive?
1. Alkali metals(g1) 2. Alkaline earth metals(g2)
3. Halogens(g17)
4. Noble gases(g18)
26. The distance between two consecutive peaks or troughs in a wave is:
1. valence shell
2. quantum number
3. amplitude
4. wavelength
27. When electrons in an atom, ion, or molecule have the lowest possible energy, they are
said to be in:
1. ground state
2. degenerate orbitals
3. s orbital
4. polyatomic ions
28. Using a periodic table, which element is classified as a non-metal?
1. Au
2. I
3. Y
4. V
29. Elements in the same group of the periodic table have the same
1. number of valence electrons
2. physical properties
3. number of electrons
4. electron configuration
30. The element nitrogen is classified as a:
1. nonmetal
2. metalloid
3. metal
4.transition metal
31. Which of the following ions is correct?
1. Cl⁺ 2. Ca⁺ 3. O²⁺ 4. Mg²⁺
32. Which element requires the least amount of energy to remove an electron to form an
ion?
1. Na 2. Ar 3. P 4. Cl
33. An orbital is a region in an atom where there is a high probability of finding
1. an alpha particle 2. an electron 3. a neutron 4. a proton
34. Which element is classified as a metalloid?
1. boron 2. potassium 3. sulfur 4. xenon
35. What is the number of electrons shared between the atoms in a molecule of nitrogen,
N₂?
1. 8 2. 2 3. 3 4. 6
36. Given the equation representing a reaction:
H + H --> H₂
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What occurs during this reaction?
1. A bond is broken and energy is absorbed.
2. A bond is broken and energy is released.
3. A bond is formed and energy is absorbed.
4. A bond is formed and energy is released.
37. An atom of which element has the strongest attraction for electrons in a chemical bond?
1. chlorine 2. carbon 3.phosphorus 4. sulfur
38. When a sample of Mg reacts completely with O₂, the Mg loses 5.0 moles of
electrons.How many moles of electrons are gained by the O₂?
1. 1.0 mol 2. 2.5 mol 3. 5.0 mol 4. 10.0 mol
39. Which compound has covalent bonds?
1. H₂O 2. Li₂O 3. Na₂O 4. K₂O
40. The mass of an electron is
1. equal to the mass of a proton
2. equal to the mass of a neutron
3. greater than the mass of a proton 4. less than the mass of a neutron
41. Which ion in the ground state has the same electron configuration as an atom of neon in
the ground state?
1. Ca²⁺ 2. Cl⁻ 3. Li⁺ 4. O²⁻
42. Valence electrons are electrons that are
1. in the ground state
2. in the highest energy level
3. in an excited state
4. in a shielding energy level
43. Which of the following compounds has a linear structure?
1. H₂O 2. NH₄⁺ 3. CO₂ 4. NO₂⁻
44. When comparing the H-N-H bond of NH₃, and the H-C-H of CH₄, the H-N-H bond angle is
1. the same 2. larger 3. smaller 4. cannot determine
45. Which of the following atoms would be expected to form negative ions in binary ionic
compounds?
1. K 2. I 3. Q 4 Co
46. Identify the most polar bond
1. Se - H 2. C - H 3. C - C 4. O - H
47. Which of the following formulas has a total of 32 valence electrons spread out among its
entire structure?
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1. HONO
2. PO₄³⁻
3. ICl₄⁻
4. SO₃²⁻
48. Binary ionic compounds are composed of two elements, they are usually:
1. two nonmetals 2. two metals 3. a metal and a non metal 4 all options are viable
49. The formal charge of an atom in a molecule is the ____ charge the atom would have if we
could redistribute the electrons in the bonds evenly between the atoms.
1. actual 2. hypothetical 3. negative 4. positive
50. Which terms identify two different categories of compounds?
1. covalent and molecular 2. covalent and empirical
3. ionic and molecular
4. ionic anc empirical
51. Which part of a calcium atom in the ground state is represented by the dots in its Lewis
electron dot diagram?
1. the electrons in the first shell 2, the electrons in the fourth shell
3. the protons in the nucleus 4. the neutrons in the nucleus
52. Which element has chemical properties that are most similar to potassium?
1. calcium 2. cesium 3. nitrogen 4. sulfur
53. Which substance can not be broken down by chemical means?
1. aluminum 2. ammonia 3. aluminum oxide 4. ammonium chloride
54. Magnesium and calcium have similar chemical properties because their atomsin the
ground state have
1. equal numbers of protons and electrons
2. equal numbers of protons and neutrons
3. two electrons in the first shell
4. two electrons in the outermost shell
55. What is the percent composition by mass of nitrogen in the compound N₂H₄(gramformula mass = 32 g/mol)?
1. 13% 2. 44% 3. 88% 4. 93%
56. What is the number of electrons in a completely filled second shellof an atom?
1. 32 2. 2 3. 18 4. 8
57. As a result of the gold foil experiment, it was concluded that an atom
1. contains protons, neutrons, and electrons
2. contains a small, dense nucleus
3. has positrons and orbitals
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4. is a hard, indivisible sphere
58. Which sample of matter is classified as a substance?
1. air 2. milk 3. ammonia 4. seawater
59. Which sample of CO₂ has a definite shape and a definite volume?
1. CO₂(aq) 2. CO₂(g) 3. CO₂(l) 4. CO₂(s)
60. Which statement describes a chemical change?
1. Alcohol evaporates.
2. Water vapor forms snowflakes.
3. Table salt (NaCl) is crushed into powder.
4. Glucose (C₆H₁₂O₆) and oxygen produce CO₂ and H₂O.
61. Which quantity is equal to 50 kilojoules?
1. 0.05 J 2. 500 J 3. 5 X 10³ J 4. 5 X 10⁴ J
62. Which element is paired with an excited-state electron configuration for an atom of the
element?
1. Ca: 2-8-8-2 2. Na: 2-8-2 3. K: 2-6-8-3 4. F: 2-8
63. An ion that consists of 7 protons, 6 neutrons, and 10 electrons has a net charge of
1. 4- 2. 3- 3. 3+ 4. 4+
64. Which quantity can vary among atoms of the same element?
1. mass number 2. atomic number 3. number of protons 4. number of electrons
65. Compared to the energy and charge of the electrons in the first shell of a Be atom, the
elecrtrons in the second shell of this atom have
1. less energy and the same charge
2. less energy and a different charge
3. more energy and the same charge
4. more energy and a different charge
66. In a bond between an atom of carbon and an atom of fluorine, the fluorine atom has a
1. weaker attraction for electrons
2. stronger attraction for electrons
3. smaller number of first-shell electrons
4. larger number of first-shell electrons
67. An effective collision between reactant particles requies the particles to have the proper
1. charge and mass 2. charge and orientation
3. energy and mass 4. energy and orientation
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Winter Homework
68. Two grams of potassium chloride are completely dissolved in a samaple of water in a
beaker.This solution is classified as
1. an element 2. a compound
3. a homogeneous mixture 4. a heterogeneous mixture
69. As the elements in Period 3 are considered in order of increasing atomic number, there
is a general decrease in
1. atomic mass 2. atomic radius
3. electronegativity 4. first ionization energy
70. Which compound has the highest percent composition by mass of strontium?
1. SrCl₂ 2. SrI₂ 3. SrO 4. SrS
71. Which term identifies a form of energy?
1. combustion 2. exothermic 3. thermal
4. electrolytic
72. Which substance forms an unsaturated solution when 80 grams of the substance are
stirred into 100 grams of water at 10degrees C?
1. KNO₃ 2. KI 3. NH₃ 4. NaCl
73. Which element tends to NOT react with other elements?
1. helium 2. hydrogen 3. phosphorus 4. potassium
74. The joule is a unit of
1. concentration 2. pressure
3. volume
4. energy
75. Given the balanced equation representing a reaction:
2NO + O₂ → 2NO₂ + energy
The mole ratio of NO to NO₂ is
1. 1 to 1 2. 2 to 1 3. 3 to 2 4. 5 to 2
True / False:
76. [ T | F ] Electron affinity is the energy change for the process of adding an electron to a
gaseous atom to form a cation.
77. [ T | F ] Metal atoms are more likely to become positive ions in chemical reactions than
nonmetal atoms.
78. [ T | F ] Fluorine has the largest electron affinity.
79. [ T | F ] The bond that joins Na and Cl in NaCl is an ionic bond.
Winter Homework
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80. [ T | F ] The element Sc has a larger atomic radius than the element As.
81. [ T | F ] All ionic compounds include at least one metal and one non-metal elements.
82. [ T | F ] An Al³⁺ ion has a larger atomic radius than a S²⁻ ion.
83. [ T | F ] In ordinary chemical reactions, the nucleus of each atom changes when bonding
occurs.
84. [ T | F ] Classical physics does not accurately explain the behavior of electrons, and a
new type of physics was created.
85. [ T | F ] Plank's constant 'h' will change when describing electrons in different energy
states.
86. [ T | F ] removing an electron from a cation is generally easier than an atom of the same
element because there are fewer electrons.
87. [ T | F ] When electrons fill orbitals, they will fill available unoccupied sub orbitals of the
same energy before pairing with other electrons in a single suborbital.
88. [ T | F ] polyatomic ions react with other elements to form covalent molecules.
89. [ T | F ] Non-metal elements generally form negatively charged ions.
90. [ T | F ] The compound CH₄ has the same electron pair geometry and molecular
geometry.
91. [ T | F ] Atoms share electrons when they undergo covalent bonding,
92. [ T | F ] A single covalent bond contains 1 electron.
93. [ T | F ] Ionic compounds are not molecules.
94. [ T | F ] Electron density in a triple bond takes up more space than the electron density
of lone pair electrons.
95. [ T | F ] Polar molecules contain at least one polar bond.
96. [ T | F ] Non-polar molecules do not contain any polar bonds.
97. [ T | F ] Lewis structures depict core electrons to calculate electron shielding.
Winter Homework
98. [ T | F ] A cation gains proton to form a positive charge.
99. [ T | F ] Br is more electronegative than Cl
100.
[ T | F ] A cation gains it's charge by adding a proton
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