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General Chemistry
General Chemistry
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1
How many grams of NaOH (40 g/mol) is needed to prepare 500 mL 0f 0.500M solution of NaOH?
4g
5g
10 g
10.3 g
2
As you move from right to left across a period in the periodic table, what generally happens to the ionization energy?
Increases
Fluctuates
Remains constant
Decreases
3
What does ionization energy refer to?
Energy needed to bond two atoms
Energy needed to add a proton
Energy needed to remove an electron
Energy needed to create an ion
4
Which of the following statements is TRUE?
None of the statements is TRUE
Single bonds have lower energy than double bons.
Double bond are stronger than triple bonds
Double bonds are shorter than triple bonds
5
What is the charge of the cyanide ion?
0
-1
+1
+2
6
According to Thomson's Plum Pudding model:
Atoms like pudding with electrons
Atoms indivisible
Atoms nucleus and electrons
Atoms mostly empty space
7
What is the molar mass of carbon dioxide (CO2)?
28 g/mol
12 g/mol
44 g/mol
16 g/mol
8
The standard pressure of the atmosphere at sea level is?
all of the above
760 mmHg
760 torr
1 atm
9
Which of the following is NOT a physical property of matter?
Flammability
Melting point
Electrical conductivity
Density
10
A solution is ______ if more solute can dissolve in it.
saturated
concentrated
supersaturated
unsaturated
11
How many atoms are in one mole of a substance according to Avogadro's number?
1
10
100
6.02 x 10^23
12
Chromium is a member of which of the following?
lanthanides
Alkali metals
Transition Metals
Actinides
13
In Rutherford's Nuclear Model of the atom:
Atoms like a tiny solar system
Atoms indivisible
Atoms have a nucleus
Atoms mostly empty space
14
Which element is present in cyanide compounds?
Oxygen
Carbon
Helium
Sodium
15
It is the process that changes the physical properties of a substance without changing its chemical composition.
Physicochemical change
biological change
Physical change
Chemical change
16
Which of the following atoms is the largest?
Strontium (Sr)
Gallium (Ga)
Cesium (Cs)
Arsenic (As)
17
Which element has the highest electronegativity on the periodic table?
Oxygen
Fluorine
Chlorine
Nitrogen
18
Which of the following is NOT an indication of strong IMFA?
High viscosity
High boiling point
High melting point
High votality (easily evaporated)
19
Isotopes of an element have the same number of:
Electrons
Valence electros
Neutrons
Protons
20
It is the process in which one or more substances are converted into one or more new substances.
Biological change
Physical change
Physicochemical change
Chemical change
21
What is the mass of flouride (19 g/mol) in 24.6 g of Tin (II) flouride (156.7 g/mol)?
0.31 g
101.4 g
5.97 g
2.98 g
22
How many moles of carbon atoms are present in 12 grams of carbon (C)?
2 moles
0.5 moles
1 mole
3 moles
23
Which does NOT indicate a chemical change?
increase in temperature
change in color
change in shape
evolution of gas
24
1.00 g sample of which compound will produce the greatest amount of CO2 after complete combustion with excess oxygen.
C8H18 (Saturated, Octane)
C6H14 (Saturated, 1-Methylcycloheptene)
C3H6 (Unsaturated, propene)
CH4 (Methane)
25
Density is ___________.
the amount of matter in the object.
The amount of space the object occupies.
None of the choices.
The amount of mass per unit volume.
26
From left to right in a periodic table ___________.
none of the above
atomic radius increases
electronegativity increases
ionization energy decreases
27
hat do Lewis structures represent in chemistry?
Electron arrangement in molecules
Temperature of substances
Proton arrangement in atoms
Density of compounds
28
Which of the following is an example of a chemical property?
reactivity with acid
density
boiling point
color
29
What does the term "molar mass" represent in chemistry?
Mass of one mole of a substance
Density of a substance
Volume of one mole of a substance
Number of atoms in a substance
30
What type of bond forms between two nonmetal atoms that share electrons?
metallic
covalent
hydrogen
Ionic
31
Which procedure produces a 0.2M solution of Na2SO4?
Diluting 400 mL of 0.3M Na2SO4 to a final volume of 1.0L.
Mixing 300 mL of 1.2 NaOH with 600 mL of 0.3 M Na2SO4.
Mixing 500 mL of 0.4M NaOH with 500 mL of 0.2M Na2SO4.
Dissolvong 0.2M solid Na2SO4 in 500 mL water.
32
What is a binary ionic compound composed of?
Only one element
Two nonmetals
Two metals
A metal and a nonmetal
33
In Bohr's Planetary Model:
Atoms mostly empty space
Atoms like a mini solar system
Atoms indivisible
Atoms have electron orbits
34
The flask in the image above (1, 2, and 3) contains the same no. of molecules. In which flask is pressured the highest?
Flask 2
Flask 3
All of them have the same pressure
Flask 1
35
What unit is molar mass typically expressed in?
L
Kg
mol
g/mol
36
Which statement is TRUE?
The value of the equilibrium constant rises with the addition of a catalyst
The greater the activation energy, the faster the rate of reaction.
a catalyst speeds up both the forward and reverse reaction rates.
A catalyst rises the rate of reaction by decreasing the no. of collisions
37
Which intermolecular force is the strongest among the listed options?
Hydrogen bonding
Dipole-dipole interaction
London dispersion force
Ionic bonding
38
Isotopes are atoms that have:
Same atomic mass
Same number of protons
Same number of neutrons
Different number of neutrons
39
What does the empirical formula of a compound represent?
Simplest whole-number ratio of atoms
Molecular weight
Total number of atoms
Number of moles
40
Which of the following is an extensive property of matter?
number of moles
density
viscosity
freezing point
41
What is the standard atmospheric pressure at sea level?
1 atm
All of the above
760 mmHg
101.3 kPa
42
The empirical formula of a compound is CH. the molar mass of the compound is 78 g/mol, what is its molecular formula?
None of the above.
C8H8 (Styrene)
C2H2 (Acytelene)
C6H6 (Benzene)
43
What does the octet rule state regarding the electron configuration of atoms?
Atoms cannot form chemical bonds
Atoms can have any number of electrons in their outer shell
Atoms need to have eight electrons in their outer shell to be stable
Atoms must donate all their electrons to other atoms
44
What is the principal intermolecular force that must be overcome when hexane is vaporized?
London dispersion forces
Hydrogen bonding
Dipole-dipole forces
Covalent bonding between Carbons
45
Flourine is capable pf forming covalent bonds with which of the following element?
Zinc (Zn)
Lithium (Li)
Boron (B)
Calcium (Ca)
46
Which of the following is NOT an acid-based conjugate pair?
HCN (Hydrogen cyanide) and CN- (Cyanide)
H2S (Hydrogen sulphide) and OH- (Hydroxide)
H2O (water) and OH- (Hydroxide)
NH3 (ammonia) and NH4 (ammonium)
47
Which of the following is TRUE?
Heteregeous mixtures have phase boundaries.
Solutions are considered as pure substances
Elements can be chemically decomposed.
Compounds have only one type of atom
48
What happens to the volume of a gas if the pressure is doubled, according to Boyle's Law?
The volume remains the same
The volume is halved
The volume is doubled
The volume is quadrupled
49
For which compound are the empirical and molecular formulas the same?
HOOCCOOH (Oxalic acid)
C6H4(COOH)2 (Phthalic acid)
CH3COOH (Acetic acid)
C6H5COOH (Benzoic acid)
50
Which of the following does NOT describe a nonpolar bond?
It is a bond between similar nonmetals
It has a dipole moment
All describes a nonpolar bond.
It is a bond between different nonmetals
51
A polar solute dissolves in a polar solvent and nonpolar dissolve in a nonpolar solvent. This is the _____________.
Solubility rule
Hunds' rule
Henrys Law
Like Dissolves like' rule
52
Which of the following is a physical property of matter?
Reactivity with oxygen
Mass
Toxicity
Flammability
53
What determines the shape of a molecule in molecular geometry?
Number of neutrons
Arrangement of atoms
Color of the compound
Size of the molecule
54
Which of the following is an intensive property?
melting point
all of the above
electric potential
density
55
The synthesis og NH3 from N and H is an exothermic reaction. Which of the following will favor the formation of ammonia?
addition of ammonia
removal of nitrogen
decrease in temperature
increase in temperature
56
Which of the following is a chemical equation?
C + O2 = CO2
Iron + Oxygen = Rust
CO2
Ice + heat = Water
57
Which factor determines the atomic radius of an atom?
Atomic mass
Number of electron shells
Number of protons
Number of neutrons
58
Which group of elements in the periodic table typically has the lowest ionization energy?
Alkali metals
Transition metals
Halogens
Noble gases
59
What type of bond involves the sharing of electrons between atoms?
ionic
covalent
metallic
hydrogen
60
Whic of these elements are strict followers of the octet rule, EXCEPT
Boron (B)
Nitrogen (N)
Carbon (C)
Oxygen (O)
61
What is the term used to describe the attraction between water molecules due to hydrogen bonding?
Adhesion
Surface tension
Cohesion
Capillarity
62
What property determines whether a molecule is polar or nonpolar?
Atomic mass
Electronegativity difference
Melting point
Number of protons
63
What type of intermolecular force is present in molecules with hydrogen bonded to Fluorine, Oxygen, or Nitrogen?
Hydrogen bonding
Ionic bonding
Dipole-dipole interaction
London dispersion force
64
What is the molar mass of water (H2O)?
12 g/mol
18 g/mol
24 g/mol
36 g/mol
65
What type of intermolecular force occurs between polar molecules?
London dispersion force
Dipole-dipole interaction
Ionic bonding
Hydrogen bonding
66
Which intermolecular force is the weakest and present in all molecules?
Dipole-dipole interaction
London dispersion force
Hydrogen bonding
Ionic bonding
67
Which trend does the atomic radius follow as you move from left to right across a period in the periodic table?
Remains constant
Fluctuates
Increases
Decreases
68
Which compound has the strongest intermolecular forces of attraction?
CH3OCH3 (Methoxy methane)
CH4 (Methane)
CH3OH (Methanol)
CO (Carbon monoxide)
69
Polar molecules include which of the following?I. CO2 II. COCl2 (Phosgene)III. CH2Cl2 (Dichloromethane)
1 only
I and III only
I and II only
II and III only
70
Which of the following can change the value of the equilibrium constant?
addition of a catalyst
change in pressure or volume
change in concentration
change in temperature
71
Mass ____________________.
form the force exerted on matter by the gravitational attraction of earth.
is the quantitative measure of acceleration, a prime property of all matter
has the SI unit of pounds.
is the amount of matter that occupies space.
72
What happens to the volume of a gas if temperature is doubled while keeping the pressure constant through Charles' law?
The volume quadruples
The volume is halved
The volume is doubled
The volume remains the same
73
Which of the following is a polar molecule?
XeF4 (Xenon Tetraflouride)
CO2 (Carbon dioxide)
CCl4 (Carabon tetrachloride)
SF4 (Sulfur tetraflouride)
74
According to Dalton's Billiard Ball model:
Atoms are mostly empty space
Atoms have a nucleus and electrons
Atoms are indivisible
Atoms are like tiny billiard balls
75
How does electron affinity generally change as you move from left to right across a period in the periodic table?
Remains constant
Varies unpredictably
Decreases
Increases
76
Which is NOT an acceeptable name gor Hg2Cl2?
Dimercury dichloride
Mercury (II) chloride
Mercury (I) chloride
Mercurous chloride
77
Which of the following is described as having components that CANNOT be physically separated?
suspension
solution
mixture
pure substance
78
The lining of the stomach contains cells that secrete a solution of HCl. Which drink would best alleviate heartburn?
milk of magnesia (pH 10.5, Mg(OH)2)
wine (pH 3.8)
milk (pH 6.5)
diet soda (pH 4.3)
79
Which of the following instruments is used to measure atmospheric pressure?
Hygrometer
Anemometer
Barometer
Thermometer
80
Which of the following covalent compounds has a tetrahedral geometry?
H2O (2 lone pair, Water)
BF3 (0 lone pair, Boron triflouride)
NH3 (1 lone pair, Ammonia)
CH4 (0 lone pair, Methane)
81
When Ammonium chloride undergoes ionization, the resulting solution will have a pH______?
7
>7
<7
14
82
How does the molar mass of a compound relate to its chemical formula?
It provides the ratio of elements in the compound.
It specifies the temperature at which the compound boils.
It indicates the number of moles in the compound.
It determines the state of matter of the compound.
83
What is the chemical formula of Diphosphorus monobromide?
P2Br2 (Diphosphorous dibromide)
P2Br (Diphosporous monobromide)
PBr (Phosphorous bromide)
PBr2 (Phosphorous dibromide)
84
Upon using MOTHBALLS in air for a few hours, they disappeared. Which of the following BEST explains the scenario.
evolution of gas
It underwent sublimation.
It melted then vaporized
It reacted with something in the air
85
Which of the following factors affects the ionization energy of an atom?
Atomic mass
Number of neutrons
Atomic number
Number of electron shells
86
What does electronegativity measure?
Number of protons in an atom
Atom's ability to repel electrons
Atomic mass
Atom's ability to attract electrons
87
According to Avogadro's Law, at constant temperature and pressure, which relationship holds true for gases?
The volume of a gas is directly proportional to its temperature
The volume of a gas is inversely proportional to its pressure
The volume of a gas is directly proportional to the number of moles of gas
The volume of a gas is inversely proportional to its temperature
88
What does Electron affinity measure?
Attraction of an atom for an electron
Number of electrons in an atom
Repulsion of an atom for an electron
Stability of an atom
89
Which of the following is TRUE for C-13 isotope?
It has 6 protons and 7 neutrons
It has 6 neutron and 13 protons
It has 6 protons and 13 neutrons
It has 6 neutron and 7 protons
90
Noble gasses are unreactive because they have complete outer electron shell. Which of the following is NOT a noble gas?
Chlorine (Cl)
Helium (He)
Krypton (Kr)
Argon (Ar)
91
What is the molar mass of an unknown gas if 1.60g of the gas occupies a volume of 2.24L at stp?
160 g/mol
35.8 g/mol
81.0 g/mol
16.0 g/mol
92
What is the most common isotope of Hydrogen?
Tritium (H-3)
Protium (H-1)
hydrogen only has one isotope
Deuterium (H-2)
93
What element is always present in oxyacids?
Nitrogen
Carbon
Oxygen
hydrogen
94
Which property of an atom determines its chemical behavior?
Number of protons
Atomic number
Number of electrons
Atomic mass
95
Which of the following is a characteristic of transition metals?
Non-reactive with other elements
Found in Group 1 of the periodic table
Variable oxidation states
Only one stable isotope
96
How is the molar mass of a compound calculated?
By dividing the mass by the number of moles
By multiplying the mass by Avogadro's number
By counting the number of atoms in the compound
By summing the atomic masses of all the atoms in the compound
97
Which of the following statements best describes viscosity?
Viscosity is the ability of a liquid to evaporate quickly.
Viscosity is the measure of a liquid's transparency.
Viscosity is a measure of a liquid's resistance to flow.
Viscosity is the amount of solute that can dissolve in a solvent.
98
Which statement is TRUE about mixture?
All statement are TRUE
It is the simplest substances.
It consist of two or more elements or compounds.
It cannot be physically separated.
99
What type of bond forms between elements in an ionic compound?
Metallic
Ionic
Hydrogen
Covalent
100
Sodium Carbonate (NaCO3) is also known as?
Baking soda (NaHCO3, Sodium bicarbonate)
Soda Ash
Caustic potash (KOH, Potassium hydroxide)
Caustic soda (NaOH, Sodium hydroxide)
