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Chemistry study guide final project
Chemistry study guide final project
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1
A student measures 48 mL of water instead of the accepted 50 mL. What is the percent error?
0.5%
4%
5%
2%
2
Which metric conversion is correct?
1 meter = 1000 kilometers
1 kilometer = 100 meters
1 centimeter = 100 meters
1 millimeter = 0.001 meter
3
Which of the following polyatomic ions is hydroxide?
NH4+
NO3⁻
PO43-
OH⁻
4
What subatomic particles are found in the nucleus of an atom?
Neutrons and electrons
Protons and neutrons
Electrons only
Protons and electrons
5
What is a mole ratio in a chemical reaction?
Ratio of mass to volume
Ratio of reactants to products by grams
Ratio of coefficients in a balanced equation
Ratio of atoms in a compound
6
What type of compound is formed when two nonmetals bond?
Ionic
Covalent
Hydrogen
Metallic
7
Which of the following is a characteristic of a Bronsted-Lowry acid?
Produces H2 gas
Increases [OH⁻] in water
Accepts OH- ions
Donates H+ ions
8
Which model of the atom did John Dalton propose?
Solid sphere model
Plum pudding model
Planetary model
Nuclear model
9
Which particle has a negative charge?
Proton
Electron
Gamma ray
Neutron
10
Which elements are always found as diatomic molecules in nature?
Group 1 metals
BrINClHOF
Noble gases
Transition metals
11
What does it mean if your measurements are precise but not accurate?
They are always wrong
They are all different
They are close to the true value
They are close to each other but not the accepted value
12
What is the formula for ammonium carbonate?
NH4(CO3)2
NH42CO3
(NH4)2CO3
NH3CO3
13
Which acid has the formula HNO
3
?
Acetic acid
Nitric acid
Hydrochloric acid
Sulfuric acid
14
What distinguishes an isotope from a regular atom of the same element?
Different number of neutrons
Different number of electrons
Different number of protons
15
What is the pOH of a solution with a pH of 5?
14
7
5
9
16
Which of the following is true about isotopic notation
14
6
C
Mass number = 6
Mass number = 14
Atomic number = 14
It has 6 neutrons
17
How many atoms are in the formula H
2
SO
4
?
5
6
4
7
18
Which element is a noble gas?
Fluorine
Sodium
Argon
Beryllium
19
What happens to the pressure of a gas if the volume decreases and temperature remains constant?
Moles of gas decrease
Pressure increases
Pressure stays the same
Pressure decreases
20
If you are given grams of both reactants, what should you do first to find the limiting reactant?
Add the masses
Find the product’s mass
Convert both to moles
Subtract the smaller from the larger
21
What is the mass of NaCl needed to make 0.5 L of 1 M solution? (Molar mass of NaCl = 58.5 g/mol)
116.0 g
14.6 g
29.25 g
58.5 g
22
Which of the following is a neutralization reaction?
CH4 + O2 --> CO2 + H2O
HCl + NaOH --> NaCl + H2O
Na + Cl2 --> NaCl
CaCO3 --> CaO + CO2
23
If 3 moles of nitrogen react with excess hydrogen in the reaction N
2
+ 3H
2
--> 2NH
3
, how many moles of NH
3
are produced?
3
2
6
1
24
What major discovery is Thomson known for?
The electron
The neutron
The proton
The nucleus
25
Which equation is correctly balanced?
2H2 + O2 --> 2H2O
H2 + O2 --> 2H2O
H2 + 2O2 --> 2H2O
H2 + O2 --> H2O
26
What is the strongest type of intermolecular force?
Ionic Bond
Dipole-Dipole
Hydrogen Bonding
Dispersion
27
Which type of bond is the strongest and shortest?
Single
Triple
Quadruple
Double
28
What is the correct shape of CO
2
?
Tetrahedral
Bent
Linear
Trigonal Pyramidal
29
What type of reaction is: AB + CD --> AD + CB?
Decomposition
Single Replacement
Double Replacement
Synthesis
30
Which of the following is a correct conversion from Celsius to Kelvin?
K = C x 273
K = C − 273
K = C / 273
K = C + 273
31
Which statement best describes nuclear fusion?
Two small nuclei combine to form a larger nucleus
An atom loses an electron to become an ion
A large nucleus splits into smaller nuclei
A neutron changes into a proton inside the nucleus
32
Which of the following elements has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁵?
Neon
Chlorine
Fluorine
Oxygen
33
What is Avogadro’s number?
3.14 x 106
1.67 x 10-27
6.022 x 1023
6.022 x 1022
34
Which of the following is not a gas law?
Charles’ Law
Gay-Lussac’s Law
Newton’s Law
Combined Gas Law
35
Which of the following elements is diatomic in its natural form?
Nitrogen
Sodium
Helium
Carbon
36
Which element can be an exception to the octet rule?
Carbon
Fluorine
Nitrogen
Boron
37
In a single replacement reaction, what is needed to determine if a reaction will occur?
Activity series
Molar mass
Temperature
Color of the compounds
38
Which of the following is a synthesis reaction?
AB --> A + B
A + BC --> AC + B
AB + CD --> AD + CB
A + B --> AB
39
A solution with a pH of 3 is best described as...
Strong acid
Weak base
Strong base
Neutral
40
Which type of reaction is this? CaCO
3
--> CaO + CO
2
Combustion
Synthesis
Double Replacement
Decomposition
41
In a saltwater solution, which is the solute?
Both salt and water
Air
Water
Salt
42
Which of the following has the highest electronegativity?
Sodium
Carbon
Fluorine
Aluminum
43
What type of nuclear radiation can be stopped by a sheet of paper?
Gamma
Protons
Alpha
Beta
44
What is the product of a combustion reaction involving a hydrocarbon?
O2 and H2
CO2 and H2O
NaCl and CO2
HCl and H2O
45
What is percent yield?
Reactant mass x product mass
Actual yield / theoretical yield x 100
Actual yield – theoretical yield
Theoretical yield / actual yield × 100
46
What is the mass of one mole of carbon atoms?
12.01 g
1.008 g
12.01 amu
6.022 g
47
What is the unit for molar mass?
mol/g
g/mol
kg/mol
amu
48
What is the definition of pH?
Partial hydrogen
Percent hydrogen
Power of hydroxide ions
Power of hydrogen ions
49
What do all elements in the same group (column) have in common?
Same number of valence electrons
Same mass
Same number of protons and neutrons
Same atomic number
50
Which molecule shows hydrogen bonding?
CO2
CH4
H2O
HCl
51
What do you need to convert grams to moles?
Density
Volume
Molar mass
Temperature
52
How is the periodic table arranged?
By increasing atomic mass
By increasing number of neutrons
By increasing atomic number
By alphabetical order
53
In the Ideal Gas Law
PV = nRT
what does ‘n’ represent?
Moles of gas
Temperature
Pressure
Volume
54
What happens to atomic radius as you move from left to right across a period?
Increases
Changes randomly
Decreases
Stays the same
55
What does Charles’ Law state about volume and temperature of a gas?
Volume stays the same as temperature increases
Volume increases as temperature increases
Volume and temperature are inversely related
Volume is constant when temperature changes
56
Which factor affects a molecule’s melting or boiling point?
Color of the substance
Polarity and intermolecular forces
Mass of atoms only
Type of chemical bond only
57
Which of the following is an indicator of a chemical reaction?
Change in shape
A change in size
Melting of a solid
Formation of a new substance
58
What is the correct name for ZnCl
2
?
Zinc dichloride
Zinc(II) chlorate
Zinc chloride
Zinc(II) dichloride
59
Which statement about dipole-dipole forces is true?
They are weaker than dispersion forces.
They occur between polar molecules
They only occur between nonpolar molecules.
They occur in all molecules.
60
Which of the following has the smallest mass?
All are equal
Electrons
Neutron
Proton
61
In a balanced chemical equation, coefficients represent:
Number of molecules
Volume of gases
Number of moles
Grams of each substance
62
How does increasing temperature affect gas particle movement?
Particles slow down
Particles move faster
Particles become heavier
Particles stick together
63
Which of the following is a correct definition of
limiting reactant
?
The reactant that gets used up first and limits how much product forms
The one left over after the reaction
The one that produces the most product
The reactant that is in the smallest container
64
Which part of the atom is involved in chemical bonding?
Electrons
Protons
Valence electrons
Neutrons
65
If an atom absorbs energy, its electrons will...
Move to a higher energy level
Drop to a lower energy level
Leave the atom permanently
Become neutrons
66
Which of the following is a property of metallic bonding?
Free-flowing sea of electrons
Low melting point
Electrons shared between two nonmetals
Brittle
67
What is the correct word equation for the formula: Na + Cl
2
--> NaCl?
Chlorine reacts with salt
Sodium and chlorine decompose to form sodium chloride
Sodium reacts with sodium chloride
Sodium reacts with chlorine to produce sodium chloride
68
According to Bohr’s atomic model, electrons...
Stay still inside the atom
Are a mindset
Float randomly around the nucleus
Orbit the nucleus in specific energy levels
69
Which of the following best describes ionic compounds?
Soft, malleable, conducts electricity
Usually gases at room temperature
High melting point, brittle, electrically neutral
Low melting point, poor conductor
70
Which law explains the inverse relationship between pressure and volume?
Gay-Lussac’s Law
Boyle’s Law
Charles’ Law
Ideal Gas Law
71
Why is titration useful in chemistry?
To create acids
To make gases
To separate mixtures
To determine unknown concentrations
72
In the equation: 2H
2
+ O
2
--> 2H
2
O, what is the mole ratio of H
2
to H
2
O?
2:2
2:1
1:2
1:1
73
Which group on the periodic table contains the most reactive metals?
Halogens
Alkali metals
Noble gases
Metalloids
74
What was the main flaw in Dalton’s atomic theory?
He believed atoms could be divided
He discovered the electron
He thought all atoms of an element were identical
He thought atoms were mostly empty space
75
What is the equation for Dalton’s Law of Partial Pressures?
V/T=V/T
P1V1=P2V2
P=nRT
Ptotal=P1+P2+P3+…
76
How many moles are in 36 grams of water (H
2
O)?
18 moles
1 mole
0.5 moles
2 moles
77
What does the changing of atomic models over time show?
Experiments are usually flawed
Scientists never agree on anything
Models change with new evidence
The atom doesn’t really exist
78
What do strong acids and bases do in water?
Do not dissolve
Completely dissociate
Partially dissociate
Remain mostly undissociated
79
How many atoms are in 2 moles of sodium?
3.011 x 1023
6.022 x 1023
12.044 x 1023
2.00
80
What is the molarity of a solution with 2 moles of NaCl dissolved in 1 liter of solution?
0.5 M
2 M
1 M
4 M
81
What is the term for the time it takes for half of a radioactive sample to decay?
Decay rate
Half decay
Atomic clock
Half life
82
How many electrons can the 3p sublevel hold?
2
8
6
4
83
What is the molar mass of H
2
O?
2.00 g/mol
18.02 g/mol
10.01 g/mol
20.02 g/mol
84
What is the difference between an intermolecular force and a chemical bond?
Chemical bonds are only found in water
Intermolecular forces are stronger
Intermolecular forces occur between molecules
Chemical bonds occur between molecules
85
What is the definition of theoretical yield?
The amount of product divided by the time
The amount of reactants left over
The amount of product you measure in the lab
The maximum amount of product that can be formed from given reactants
86
Which condition will cause the volume of a gas to decrease?
Increasing the number of moles
Increasing temperature
Increasing pressure
Decreasing pressure
87
If your theoretical yield is 20 g and your actual yield is 15 g, what is the percent yield?
133%
75%
25%
5%
88
How many total valence electrons are in a molecule of CH
4
?
8
12
6
4
89
What happens to atoms during a chemical reaction?
They are created
They are destroyed
They disappear
They are rearranged to form new substances
90
Which of the following is true about atomic mass and molar mass?
Molar mass only applies to compounds
Atomic mass is bigger than molar mass
They are both in amu
They are the same number but have different units
91
What is the percent composition of hydrogen in H₂O?
88.9%
10%
18.0%
11.1%
92
Identify the conjugate base in the reaction: HCl + H
2
O --> H
3
O
+
+ Cl
-
Cl-
H3O+
H2O
HCl
93
Which statement is correct about diatomic elements?
They are all metals
They are always found as single atoms
They don't exist in nature
Their molar mass is twice the atomic mass
94
Which scientist is credited with the first idea of the atom as an indestructible particle?
Democritus
Bohr
Dalton
Thomson
95
What does one mole of oxygen (O₂) molecules represent?
6.022 x 10²³ grams
6.022 x 10²³ atoms
6.022 x 10²³ electrons
6.022 x 10²³ molecules
96
Which of the following is a property of metals?
Brittle
Poor conductor
Dull
Malleable
97
What is the shape of a molecule with 3 bonding pairs and 1 lone pair?
Tetrahedral
Bent
Trigonal Planar
Trigonal Pyramidal
98
What is one assumption of the Kinetic Molecular Theory?
Gas particles lose energy when colliding
Gas particles are in constant, random motion
Gas particles have strong attractive forces
Gas particles move in circular paths
99
Which experiment led Rutherford to discover the nucleus?
Gold foil experiment
Nucleus finder experiment
Chemistry
Gravity
100
What type of bond involves the transfer of electrons?
Metallic
Hydrogen
Covalent
Ionic
