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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
1) The number 200,000 in scientific notation is
a) 20 x 106
b) 2 x 10-5
c) 2 x 105
d) 2.0 x 104
2) How many significant figures in the number 6.00 x 103?
a) 1
b) 3
c) 5
d) 6
3) Which of the following measurements contains three significant figures?
a) 200 mL
b) 20.2 mL
c) 0.02 mL
d) 200.0 mL
4) What is the density (expressed using significant figures) of an object that has a mass of 22.4 g
and a volume of 2.0 mL?
a) 44.8 g/mL
b) 11.2 g/mL
c) 11 g/mL
d) 45 g/mL
5) The observation that in every chemical or physical process energy is neither created nor
destroyed is known as
a) Law of conservation of mass
b) Law of conservation of energy
c) Law of conservation of angular momentum
d) Law of conservation of leptons
6) Conductivity is a ______________ property
a) physical
b) chemical
7) Density is a ______________ property
a) physical
b) chemical
8) Flammability is a ______________ property
a) physical
b) chemical
9) Carbon is classified as a(n) _________________.
a) element
b) mixture
c) compound
10) Methane is classified as a(n) _________________.
a) element
b) mixture
c) compound
11) Air is classified as a(n) _________________.
a) element
b) mixture
c) compound
12) A solution is
a) Homogeneous mixture
b) An element
c) An alloy
d) A heterogeneous mixture
13) When two solutions are mixed and a solid appears the following has happened
a) Precipitation
b) Ionization
c) Excitation
d) Evaporation
14) When hydrogen gas is hit with electricity it glows because
a) Its electron absorbs the energy and moves to a different energy level and returns
b) Its proton absorbs the energy and moves to a different energy level and returns
c) It loses an electron, all positive ions glow
d) Its neutron leaves the nucleus
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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
15) The atomic mass of an element represent the number of __________ in its atoms
a) # of protons
b) # of neutrons
c) # of protons and neutrons added together
d) # of electrons
Substance A
Substance B
Protons
120
120
Neutrons
122
120
16) Which is true about substances A and B?
a) A and B are isotopes of the same element
b) A and B are different elements
Electrons
120
120
c) A has a higher charge than B
d) A is more reactive than B
17) A neutral atom of calcium has 20 electrons. How many electrons does the 2+ ion of calcium
have?
a) 22
b) 20
c) 18
d) 8
18) According to their placement on the periodic table which elements would have the most
similar atomic structures?
a) Sodium and scandium
c) Sodium and potassium
b) Sodium and barium
d) Sodium and aluminum
19) The number of neutrons in an atom 55 2 5X is
a) 30
b) 55
c) 25
d) 80
20) With n representing the outermost energy level, the electron configuration for elements in
that energy level and in group 14 is
a) ns2 np1
b) ns2 np2
c) ns2 np3
d) ns2 np4
21) An alkali metal will most likely react with
a) An alkaline earth metal
b) A transition metal
c) A noble gas
d) A halogen
22) A polar covalent bond is likely to form between two atoms that
a) Are of similar size
c) Differ in state of matter
b) Differ in electronegativity
d) Have the same number of electrons
23) To draw a Lewis structure you do not need to know
a) The number of valence electrons for each atom
b) The types of atoms in the molecule
c) The number of atoms in the molecule
d) Bond energies
24) Neils Bohr’s contribution to modern atomic theory was the proposition that
a) each atom has a specific number of positive charges
b) an atom has electrons in discrete energy levels _
c) electrons have a definite mass that can be computed
d) atomic mass is determined by the number of protons and neutrons in an atom
A
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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
25) Who is considered to be the “father of the periodic table”?
a) Rutherford
b) Thompson
c) Schroedinger
26) O2, N2, Cl2, and I2 are examples of
a) Diatomic molecules
b) Compounds
d) Mendeleev
c) Atoms
d) Ionic compounds
27) Which of the following is a balanced equation?
a) C3H8(g) + O2(g) → CO2(g) + H2O(g)
b) C3H8(g) + O2(g) → 3CO2(g) + H2O(g)
c) C3H8(g) + 2O2(g) → 3CO2(g) + 4H2O(g)
d) C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) _
A
28) How many different elements are there in ammonium hydroxide? (NH 4OH)
a) 4
b) 7
c) 3
d) 10
29) How many atoms are there in ammonium hydroxide? (NH4OH)
a) 4
b) 7
c) 3
d) 10
30) Elements are arranged in the periodic table in order of increasing
a) Atomic
b) Atomic
c) Atomic
mass
weight
number
d) Reactivity
31) The element in group 2 period 4 is
a) Calcium
b) Silicon
c) Carbon
d) Zinc
32) Elements in the same group have very similar
a) Atomic
b) Properties
numbers
c) Atomic
masses
d) Name
33) The noble gases
a) Are the last column (to the right) on the periodic table
b) Do not react with other elements
c) Are the first column (on the left) on the periodic table
d) B & C
34) Halogens, like fluorine, are very reactive because
a) They want to gain an electron to complete their outer energy level
b) They want to lose an electron to complete their outer energy level
c) They want to gain a proton in their nucleus
d) They want to lose a proton from their nucleus
35) The electron configuration for Mg2+ is
a) [Ne] 3s2
b) [He] 2s2
36) The correct orbital diagram for oxygen is
a)     
b)  
1s 2s
2p
1s 2s
c) [Ne] 3s1
  
2p
d) [He] 2s2 2p6
c)  
1s 2s
 
2p
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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
37) Cations have
a) More neutrons than protons
b) More protons than electrons
c) More electrons than protons
d) Same number of neutrons, protons, and electrons
38) Which of the following cannot be broken down by ordinary chemical means?
a) Atom
b) Mixture
c) Compound
d) Water
39) What do Li, Be, C, N and F have in common?
a) They have the same number of electrons in their outermost energy level
b) They all have the same number of protons
c) They all have the same number of energy levels
d) They are the same size
40) Oxide, O2-, is called
a) An anion
b) An element
41) Ionic bonding occurs between
a) Metals and non-metals
b) Metals and metals
c) A cation
d) A halogen
c) Non-metals and non-metals
d) Non-metals and halogens
42) Using the trend in electronegativity on the periodic table, which set of elements are in order
of increasing electronegativity?
a) Fr, Co, Al, O
c) Mg, Ca, Sr, Ba
b) Cl, P, Si, Al
d) Li, F, Ca, Br
43) An octet is
a) Eight electrons in the outermost
energy level
b) Not vary stable
c) Found in all neutral atoms
d) A sea animal
44) What is the trend for atomic size as you go across the periodic table from left to right?
a) They get smaller
c) They remain the same
b) They get larger
d) There is no pattern
45) Low ionization energy means that an atom
a) Is not willing to lose its electrons
b) Is willing to lose its electrons
c) Is unstable
d) Has an octet
46) Ionic bonds are formed by
a) Sharing electrons
b) Transferring electrons
c) Non-metals
d) Noble gases
47) What piece of glassware would you use to measure volume accurately?
a) Graduated
b) Beaker
c) Test tube
cylinder
48) The name of the compound Pb(NO3)2
a) Lead nitrate
b) Lead dinitrate
d) Flask
c) Lead (II) nitrite
d) Lead (II) nitrate
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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
49) Magnesium dissolves in hydrochloric acid to produce magnesium chloride and hydrogen
gas. Which of the following represents the reactants in this reaction?
a) Magnesium and magnesium chloride
b) Hydrochloric acid and hydrogen gas
c) Magnesium and hydrochloric acid
d) Magnesium chloride and hydrogen gas
50) The equation E=mc2 shows that
a) Chemical reactions are either exothermic or endothermic
b) Mass and energy are related
c) A hypothesis may develop into a theory
d) The kinetic energy of an object relates to its motion
51) A control in an experiment
a) Are the variables that are kept the same through each trial
b) Means that the scientist has everything under control
c) Is required only if the hypothesis leads to the development of a theory
d) Allows the scientist to identify the cause of the results in an experiment
52) How many electrons are present in an atom of tin that has an atomic number of 50 and a
mass number of 119?
a) 50
b) 69
c) 119
d) 169
53) Which of the following best represents the reaction between sulfuric acid and calcium
hydroxide?
a) H2SO4 + Ca(OH)2 → CaSO4 + H2O
b) HSO4 + CaOH → CaSO4 + H2O
c) H2SO4 + Ca(OH)2 → CaSO4 + 2H2O _
d) H2SO4 + 2Ca(OH)2 → 2CaSO4 + 3H2O
54) According to its Lewis diagram, a nitrogen molecule has a —
a) bent structure and a double bond
c) polar structure and a triple bond
b) linear structure and a triple bond _
d) circular structure and an ionic bond
55) A student has one mole of a compound in a test tube. The mass of the unknown compound
is 58.5 g. The unknown compound could be:
a) CaCl2
d) CuCl
c) NaCl
b) AgNO3
56) Cobalt, a transition metal, can have an oxidation number of either 2+or 3+. Which of these
represents the two possible chemical formulas for the chemical combination of cobalt with
oxygen?
a) CoO, Co2O3 _
c) Co2O3, C o3O2
b) CoO3, Co3O2
d) CoO, Co3O2
57) Which of the following formulas are incorrect
a) Ba(OH)2
b) LiF
c) CaCl
d) K2O
58) Which compound is covalent?
a) NH4OH
b) N2O4
c) KCl
d) MgO
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Chemistry 1 Semester Exam (A)
Name:_________________________________
Date: _______________________
59) Which of the following has the empirical formula CH 2?
a) C2H6
b) H2CO3
c) C6H6
d) C6H12
60) Choose the false statement
a) 1 mol = 6.022 x 1023 amu
b) 6.022 x 1023 atoms = 1 mole of atoms
c) 6.022 x 1023 H atoms weight 1.01 grams
d) 1 mole of carbon atoms weights 12.0 g
61) 0.314 mol of a diatomic molecule has a mass of 22.26 g. Identify the molecule
a) F2
b) Cl2
c) Br2
d) I2
62) One mole of sulfur trioxide (SO3) contains how many oxygen atoms?
a) 6.022 x 1023
b) 1.2 x 1023
c) 3.0 x 1023
63) The percent of oxygen by mass in CaO is
a) 28.5%
b) 50%
c) 72.4%
65) The charge on Manganese (VII) is ___________
a) +1
b) +7
c) +2
d) 1.8 x 1023
d) None of
the above
64) A molecule with two bonding pairs and two non-bonding pairs would be classified as what
shape?
a) Tetrahedral
b) Trigonal
c) Octahedral
d) Bent
pyramidal
d) +5
66) Which set of coefficients balances the following equation? AgCl3 + NaOH  Al(OH)3 + NaCl
a) 1, 3, 1, 3
b) 3, 1, 3, 1
c) 1, 1, 1, 3
d) 3, 1, 1, 1
67) If you start with 8 moles of water, how many moles of Hydrogen gas will you make for the
following unbalanced reaction? H2O  H2 + O2
a) 2
b) 8
c) 4
d) 6
68) You know the empirical formula for a compound. What further data do you need to
determine the molecular formula?
a) Avogadro’s number
c) The molar mass
b) The formula unit
d) The number of isotopes
69) What ions are present in K2CO3?
a) K+, C4+, O2b) K+, CO, O2 2-
c) K+, CO32d) K2+, CO32-
70) Which is the correct Lewis structure for the formula given
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