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Chemistry Final Exam Full Test
Chemistry Final Exam Full Test
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this took me so long to type out i hate this class
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1
Who arranged the elements according to atomic mass & used the arrangement to predict the properties of missing elements?
John Dalton
Henry Moseley
Antoine Lavoisier
Dmitri Mendeleev
2
What is the correct name for the N
3-
ion?
nitrite ion
nitrate ion
nitrogen ion
nitride ion
3
When an iron nail is ground into powder, its mass ____.
decreases
stays the same
cannot be determined
increasess
4
Each period in the periodic table corresponds to ____.
an energy sublevel
a suborbital
an orbital
a principal energy level
5
What are the coefficients that will balance the equation: N
2
+ H
2
→ NH
3
1,3,2
1,1,2
3,1,2
1,3,3
6
Which element, when combined with fluorine, would most likely form an ionic compound?
chlorine
phosphorous
carbon
lithium
7
When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.
-ite
-ate
-ous
-ic
8
The particles that are found in the nucleus of an atom are ___.
protons and neutrons
protons and electrons
neutrons and electrons
electrons only
9
Select the correct formula for sulfur hexafluoride.
SF6
S2F6
F6SO3
F6S2
10
Which of the following elements is in the same period as phosphorus?
nitrogen
carbon
oxygen
magnesium
11
Sulfur hexafluoride is an example of a ___.
polyatomic compound
monatomic ion
binary compound
polyatomic ion
12
Which of the following categories includes the majority of the elements?
liquids
metalloids
nonmetals
metals
13
What causes hydrogen bonding?
attraction between ions
sharing of electrons pair
bonding of covalently bonded hydrogen atom with an unshared electron pair
motion of electrons
14
In the Bohr model of the atom, an electron in an orbit has a fixed ___.
size
color
position
energy
15
What happens to matter during a chemical reaction?
Some matter is destroyed and some is created.
Some matter is created
Matter is neither destroyed or created.
Some matter is destroyed.
16
What is another name for the transition metals?
noble gases
Group A elements
Group C elements
Group B elements
17
Binary molecular compounds are made of two ___.
metallic elements
cations
nonmetallic elements
polyatomic ions
18
Which state of matter has a definite volume and takes the shape of its container?
solid
liquid and gas
liquid
gas
19
Which of the following compounds has the formula KNO
3
potassium nitrate
potassium nitride
potassium nitrogen oxide
potassium nitrite
20
The equation shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5g NO
2
is formed?
32.0 g
2.88 g
1.00 g
2.00 g
21
Which state of matter takes both thee shape and volume of its container?
solid
liquid
both liquid and gas
gas
22
Which of the following shows both the correct formula and correct name of an acid?
HNO2 ,hydronitrous acid
HClO2 ,chloric acid
H3PO4 ,phosphoric acid
HI, iodic acid
23
When x and ÷ measured quantities, the # of significant figures in the result should be equal to the # of sig. figures in
the least and most precise measurements
the most precise measurement
the least precise measurement
all of the measurements
24
What element has the electron configuration 1s²2s²2p²3s²3p²?
selenium
silver
silicon
nitrogen
25
A vapor is which state of matter?
gas
liquid
solid
all of the above
26
What are the coefficients that will balance the equation: AlCl
3
+ NaOH →Al(OH)₃ + NaCl
1,3,3,1
1,1,1,3
3,1,3,1
1,3,1,3
27
How many valence electrons are in a silicon atom?
2
6
8
4
28
Using the periodic table, determine the number of neutrons in
16
O.
24
4
16
8
29
The sum of the protons and neutrons in an atom equals the ____.
mass number
atomic number
atomic mass
nucleus number
30
In every balanced chemical equation, each side of the equation has the same number of ____.
coefficients
molecules
moles
atoms of each element
31
How many valence electrons are in an atom of phosphorus?
3
4
2
5
32
The complete combustion of which of the following substances produces carbon dioxide and water?
K2CO3
CaHCO3
NO
C8H18
33
According to the VSEPR theory, molecules adjust their shapes to keep which of the following as far apart a possible?
pairs of valence electrons
inner shell electrons
mobile electrons
the electrons closest to the nuclei
34
Elements that are characterized by the filling of s orbitals are classified as ___.
inner transition metals
groups 3A through 8A
transition metals
groups 1A and 2A
35
Who was the man who lived from 460B.C and was among the first to suggest the idea of atoms?
Thomson
Democritus
Dalton
Atomos
36
What type of ions have name ending in -ide?
only cations
only gaseous ions
only metal ions
only anions
37
What is the correct name for the compound CoCl
2
Cobalt (II) chlorate
Cobalt (I) chlorate
Cobalt(I) chloride
Cobalt(II) chloride
38
Who conducted experiments to determine the quantity of charge carried by an electron?
Rutherford
Thomson
Dalton
Millikan
39
A metallic bond is a bond between ____.
a cation and an anion
the ions of two different nonmetals
the ions of two different metals
valence electrons and cations
40
When the equation Fe + Cl
2
→ FeCl
3
is balanced, what is the coefficient for Cl
2
4
1
2
3
41
To what category of elements does an element belong if it is a poor conductor of electricity?
metalliods
metals
nonmetals
transition elements
42
Molecular compounds are usually ____.
composed of positive and negative ions
composed of two or more nonmetallic elements
exceptions to the law of definite proportions
composed of two or more transition elements
43
Which of the following compounds contains the lead (IV) ion?
PbO
Pb2S
PbO2
PbCl2
44
An example of a homogeneous mixture is
stainless steel
oxygen
water
noodle soup
45
The smallest particle of an element that retains the properties of that element is a(n) ___.
electron
neutron
atom
proton
46
This symbol (⇔) indicates that ___.
heat must be applied
the reaction is reversible
a gas is formed by the reaction
an incomplete combustion reaction has occurred
47
the modern periodic table is arranged in order of increasing atomic ____.
charge
mass
radius
number
48
An element has an atomic number of 80. The number of protons and electrons in a neutral atom of the element are ____.
80 protons and 0 electrons
160 protons and 80 electrons
80 protons and 80 electrons
40 protons and 40 electrons
49
What is the formula for sulfurous acid?
H₂SO₄
H₂SO₂
H₂SO₃
H₂S
50
How many moles of Al are needed to react completely with 1.2 moles of FeO?: 2Al + 3Fe → 3Fe + Al
2
O
3
1.2 mol
1.6 mol
2.4 mol
0.8 mol
51
When naming acids, the prefix
hydro
- is used when the name of an acid anion ends in ___.
-ite
-ate
-ide
-ic
52
The calculation of quantities in chemical equations is called ____.
dimensional analysis
stoichiometry
percent composition
percent yield
53
Dalton's atomic theory included which idea?
Individual atoms can be seen with a microscope.
All atoms of all elements are the same size.
Atoms of the same element are always identical.
Atoms of different elements always combine in one-to-one rations.
54
What is the formula for sodium sulfate?
Na2(SO4)2
Na(SO4)2
NaSO4
Na2SO4
55
In a double-replacement reaction, the ___.
products are a new element and a new compound
reactants are two elements
products are always molecular
reactants are two ionic compounds
56
Which of the following is a heterogeneous mixture?
salt water
steel
soil
air
57
The letter "p" in the symbol 4p³ indicates the ____.
spin of an electron
speed of an electron
principle energy level
orbital shape
58
The nonmetals in Groups 6A and 7A ___.
end in -ate
have a numerical charge that is found by subtracting 8 from the group #
all have ions with a -1 charge
lose electrons when they form ions
59
An -ate or -ite at the end of a compound name usually indicates that the compound contains ___.
fewer electrons than protons
a polyatomic anion
only two elements
neutral molecules
60
What hybridization occurs in the orbitals of a carbon atom participating in a single bond with another carbon atom?
sp2
pd
sp
sp3
61
All of the following are physical properties of matter EXCEPT ____.
mass
ability to rust
color
melting point
62
What causes water molecules to have a bent shape, according to the VSEPR theory?
the unusual location of the free electrons
ionic attraction and repulsion
repulsive forces between unshared pairs of electrons
interaction between the fixed orbitals of the unshared pairs of oxygen
63
What are the weakest attractions between molecules?
ionic forces
hydrogen forces
covalent forces
Van der Waals forces
64
What is the shape of a molecule with a triple bond?
tetrahedral
linear
bent
pyramidal
65
The equation 2C
3
H
7
OH + 9O
2
→ 6CO
2 +
8H
2
O
decomposition reaction
single-replacement reaction
combustion reaction
double-replacement reaction
66
A scientific law is ___.
summary of results of many observations
procedure used to test a proposed explanation
well-tested explanation for a broad set of observations
proposed explanation for an observation
67
Which of the following represents a compound?
H₂O
H-3
H
O-16
68
Which substance particle plays the greatest part in determining the properties of an element?
proton
none of the above
neutron
electron
69
The chemical symbol for iron is ___.
fe
Ir
FE
Fe
70
What are the Group 1A and Group 7A elements examples of?
nitride ion
noble gases
nonmetallic ion
representative elements
71
What is the ending for the names of all binary compounds both ionic and molecular?
-ade
-ide
-ite
-ate
72
What does the symbol Δ in a chemical equation mean?
precipitate
yields
Heat is supplied to the reaction
A catalyst is needed
73
What is the formula unit of aluminum oxide?
Al3O
Al2O3
AlO3
AlO
74
The study of the composition of matter is traditionally called what type of chemistry?
analytical
inorganic
organic
physical
75
The reaction 2Fe + 3Cl₂ → 2FeCl₃ is an example of what type of reaction?
single-replacement reaction
combustion reaction
decomposition reaction
combination reaction
76
Which of the following diatomic molecules is joined by a triple covalent bond?
N2
Cl2
He2
O2
77
All atoms of the same element have the same ____.
mass numbers
mass
number of protons
number of neutrons
78
The shape of the methane molecule is called____.
square
four-cornered
tetrahedral
planar
79
What is the charge on the strontium ion?
1-
2+
2-
1+
80
Chemical reactions _____.
only occur outside living organisms
create and destroy atoms
occur only in living organisms
produce new substances
81
What reaction takes place when one element reacts with a compound to form a new compound and a different element?
double-replacement reaction
combination reaction
decomposition reaction
single-replacement reaction
82
Which of the following compounds contains the Mn³+ ion?
MnS
MnO
MnBr₂
Mn₂O3
83
The expression of 5540 km in scientific notation is ___.
55.4 x 10⁻⁴ km
5.540 x 10⁻³ km
5.540 x 10⁴ km
5.540 x 10³ km
84
The chief advantage of the metric system over other systems of measurement is that it ____.
is in French
has more units
is in multiples of 10
is derived from nature itself
85
When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n)___.
one-sided covalent bond
unequal covalent bond
coordinate covalent bond
ionic covalent bond
86
Why do atoms share electrons in covalent bonds?
to increase their atomic numbers
to attain a noble-gas electron configuration
to become ions and attract each other
to become more polar
87
Chemical equations must be balanced to satisfy ___.
the law of definite proportions
Avogadro's principle
the law of multiple proportions
the law of conservation of mass
88
Separating a solid from a liquid by evaporating the liquid is called ____.
condensation
filtration
solution
distillation
89
Which of these elements does not exist as a diatomic molecule?
H
F
Ne
I
90
What causes dipole interactions?
attraction between polar molecules
bonding of a covalently bonded hydrogen to an unshared electron pair
attraction between ions
sharing of electron pairs
91
Why did J.J. Thomson reason that electrons must be apart of the atoms of all elements?
An electron is 2000 times lighter than a hydrogen atom.
Charge-to-mass ratio of electrons was the same, regardless of the gas used.
Cathode rays can be deflected by magnets
Cathode rays are negatively-charged particles.
92
A compound held together by ionic bonds is called a ___.
polar compound
salt
diatomic molecule
covalent molecule
93
A substance that can be separated into two or more substances only by a chemical change is a(n) ___.
solution
compound
mixture
element
