1 In the wave-mechanical model of the atom, orbitals are regions of the most probable
locations of:
(1) Protons
(2) Positrons
(3) neutrons
(4) electrons
2 Which phrase describes an atom?
(1) A positively charged electron cloud surrounding a positively charged nucleus
(2) A positively charged electron cloud surrounding a negatively charged nucleus
(3) A negatively charged electron cloud surrounding a positively charged nucleus
(4) A negatively charged electron cloud surrounding a negatively charged nucleus
3 Which total mass is the smallest?
(1) The mass of 2 electrons
(2) The mass of 2 neutrons
(3) The mass of 1 electron plus the mass of 1 proton
(4) The mass of 1 neutron plus the mass of 1 electron
4 Elements on the modern Periodic Table are arranged in order of increasing:
(1) Atomic mass
(2) Atomic number
(3) Number of neutrons
(4) Number of valence electrons
5 As the elements of Group 17 are considered in order of increasing atomic number, there is
an increase in:
(1) Atomic radius
(2) Electronegativity
(3) First ionization energy
(4) Number of electrons in the first shell
6 Chlorine-37 can be represented as
17
35Cl
37
(2) 20 Cl
(1)
(3)
(4)
35
20Cl
37
17Cl
1
7 Which element is a metal that is in the liquid phase at room temperature?
(1) Bromine
(3) hydrogen
(2) Cobalt
(4) mercury
8 Which list of formulas represents compounds, only?
(1) CO2, H2O, NH3
(2) H2, N2, O2
(3) H2, Ne, NaCl
(4) MgO, NaCl, O2
9 What is the chemical formula for iron (III) oxide?
(1) FeO
(2) Fe2O3
(3) Fe3O
(4) Fe3O2
10 An atom of which element has the greatest attraction for the electrons in a bond with a
hydrogen atom?
(1) Chlorine
(2) Phosphorus
(3) silicon
(4) sulfur
11 Which property could be used to identify a compound in the laboratory?
(1) Mass
(2) Melting point
(3) temperature
(4) volume
12 Which statement describes what occurs as two atoms of bromine combine to become a
molecule of bromine?
(1) Energy is absorbed as a bond is formed.
(2) Energy is absorbed as a bond is broken.
(3) Energy is released as a bond is formed.
(4) Energy is released as a bond is broken.
13 Given a formula for oxygen: What is the total number of electrons shared between the
atoms represented in this formula?
(1) 1
(2) 2
(3) 8
(4) 4
2
14 Solid ZnCl2 and liquid ZnCl2 have different:
(1) Empirical formulas
(2) Formula masses
(3) ion ratios
(4) physical properties
15 Which phrase describes the Molarity of a solution?
(1) Liters of solute per mole of solution
(2) Liters of solution per mole of solution
(3) Moles of solute per liter of solution
(4) Moles of solution per liter of solution
16 Which substance can not be decomposed by a chemical change?
(1) AlCl3
(2) H2O
(3) HI
(4) Cu
17 Tetrachloromethane, CCl4, is classified as a:
(1) Compound because the atoms of the elements are combined in a fixed proportion
(2) Compound because the atoms of the elements are combined in a proportion that varies
(3) Mixture because the atoms of the elements are combined in a fixed proportion
(4) Mixture because the atoms of the elements are combined in a proportion that varies
18 Which formulas represent two polar molecules?
(1) CO2 and HCl
(2) CO2 and CH4
(3) H2O and HCl
(4) H2O and CH4
19 Hydrocarbons are compounds that contain
(1) Carbon, only
(2) Carbon and hydrogen, only
(3) Carbon, hydrogen, and oxygen, only
(4) Carbon, hydrogen, oxygen, and nitrogen, only
20 The reaction that joins thousands of small, identical molecules to form one very long
molecule is called:
(1) Esterification
(3) polymerization
(2) Fermentation
(4) subs
3
21 What is the total number of protons in an atom with the electron configuration 2-8-1832-18-1?
(1) 69
(2) 79
(3) 118
(4) 197
22 Which two elements have the most similar chemical properties?
(1) Be and Mg
(2) Ca and Br
(3) Cl and Ar
(4) Na and P
23 In the ground state, each atom of an element has two valence electrons. This element
has a lower first ionization energy than calcium. Where is this element located on the
Periodic Table?
(1) Group 1, Period 4
(2) Group 2, Period 5
(3) Group 2, Period 3
(4) Group 3, Period 4
24 Which quantity identifies an element?
(1) Atomic number
(2) Mass number
(3) Total number of neutrons in an atom of the element
(4) Total number of valence electrons in an atom of the element
25 Which atom in the ground state has a partially filled second electron shell?
(1) Hydrogen atom
(3) potassium atom
(2) Lithium atom
(4) sodium atom
26 What is the total charge of the nucleus of a nitrogen atom?
(1) +5
(3) +7
(2) +2
(4) +14
27 Which value of an element is calculated using both the mass and the relative
abundance of each of the naturally occurring isotopes of this element?
(1) Atomic number
(2) Atomic mass
(3) half-life
(4) molar volume
4
28 The mass of 12 protons is approximately equal to:
(1) 1 atomic mass unit
(2) 12 atomic mass units
(3) The mass of 1 electron
(4) The mass of 12 electrons
29 Sodium atoms, potassium atoms, and cesium atoms have the same:
(1) Atomic radius
(2) First ionization energy
(3) Total number of protons
(4) Oxidation state
30 A solid substance is an excellent conductor of electricity. The chemical bonds in this
substance are most likely:
(1) Ionic, because the valence electrons are shared between atoms
(2) Ionic, because the valence electrons are mobile
(3) Metallic, because the valence electrons are stationary
(4) Metallic, because the valence electrons are mobile
31 Magnesium nitrate contains chemical bonds that are
(1) Covalent, only
(2) Ionic, only
(3) Both covalent and ionic
(4) Neither covalent nor ionic
32 Which substance can be broken down by a chemical change?
(1) Antimony
(2) Carbon
(3) hexane
(4) sulfur
5