stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
Study Guide Project - Chemistry 10 Honors Review Flashcards | StudBud
Explore
/
Study Guide Project - Chemistry 10 Honors Review
Study Guide Project - Chemistry 10 Honors Review
135 terms
·
StudBud Administration
·
1 play
Imported from external platform
Flashcards
135 cards
F
Practice quiz
P
Host live
L
Questions
135
Answers
1
UNIT 9: Define pOH
finds the basicity of a solution by measuring concentrations of OH-
measure of how acidic or basic a solution is
finds the acidity of a solution by measuring concentrations of H+
finds the charge of a solution by finding charges of OH-
2
The smallest particle in an ionic compound is a compound.
False
True
3
Silver (Ag) and zinc (Zn) typically form...
Ionic bonds
Covalent bonds
Polar bonds
Metallic bonds
4
Write the numerator of the equilibrium constant equation for: 2H2 (g) + O2 (g) ⇌ 2H2O (g)
[H2]^2[O2]
[H2O]
[H2][O2]^2
[H2O]^2
5
A solution with a pH of 7 is both basic and acidic.
False
True
6
What is the definition of chemical equilibrium?
Rates of the foward and reverse reactions are equal
The reaction stops occuring
The reaction reaches its maximum speed and then slows down
The reactants and products of an equation have the same coefficients
7
All of the following are polyatomic ions except for....
OH-
Cl-
CO3 2-
PO4 3-
8
Define a redox reaction
A reaction where electrons are lost from a substance and added to another
A reaction where a neutron collides with a uranium atom, splitting it
A reaction where electrons are gained from two substances
A reaction where electrons are attracted to each other due to no shielding
9
What is the formula for percent yield?
Percent Yield = Theoretical Yield/Actual Yield x 100%
Percent Yield = Actual Yield/Theoretical Yield x 100%
Percent Yield = Actual Yield/Theoretical Yield x 0.01
Percent Yield = Actual Yield x Theoretical Yield x 100%
10
Metals have a low ________
Boiling point
Melting point
Electrical conductivity
Insulation tendency
11
Why are noble gases generally non-reactive?
They have 1 valence electron
They have 10 valence electrons
Their outermost shell is highly unstable
They have a full outer shell
12
Electronegativity...
Decreases from left to right, increases from top to bottom
Decreases from right to left, increases from top to bottom
Increases from right to left, decreases from bottom to top
Increases from left to right, decreases from top to bottom
13
How would increasing the concentration of a reactant affect the rate of a chemical reaction?
Decrease the rate of reaction
Increase the rate of reaction
Causes fewer collisions to occur
Increases the number of particles that will repel each other
14
This characteristic, lustering, most correctly defines which of the following categories of elements?
Non-metals
Metals
Metalloids
Gases
15
Which element has the highest ionization energy?
Helium
Barium
Oxygen
Francinium
16
What phase of matter comes before the melting point?
Plasma phase
Gas phase
Liquid phase
Solid phase
17
Which of the following is an Arrhenius acid?
NH3
KOH
NaOH
HCl
18
How many significant figures are in 12.300?
Three
Five
Four
Six
19
Which of the following is an example of a heterogeneous mixture?
Air
Sugar dissolved in water
Trail mix
Saltwater
20
Identify the number of valence electrons the configuration at the very top column has.
3 valence electrons
4 valence electrons
2 valence electrons
6 valence electrons
21
An isotope has a half life of 5 years. If the initial amount was 80 g, how much of the isotope remains after 15 years?
23 g
11 g
10 g
14 g
22
Calculate the percent error if a student's result number is 22.3, while the accepted value is 20.0
2.24%
11.5%
5.55%
10.0%
23
Gay-Loussac's formula is...
P/T = P/T
PV/T = PV/T
V/T = V/T
PV = PV
24
Identify the name of the hydrate: BaCl2 * 2H2O
Monobarium chloride dihydrate
Monobarium monochloride dihydrate
Barium chloride dihydrate
Barium monochloride dihydrate
25
Water acts as a(n) _______ because it donates a proton (H+) to ammonia
Acid
Base
Solvent
Solute
26
Convert a pH of 3.5 into a [OH-]
3.16 * 10^-11
4.77 * 10^-7
2.55 * 10^-5
2.15 * 10^-10
27
UNIT 10: Which of the following is not a factor in the collision theory that affects the rate of a reaction?
Pressure
Concentration
Temperature
Orientation
28
Find the molar mass of water (H₂O)
20.03 g/mol
31.00 g/mol
34.45 g/mol
18.02 g/mol
29
UNIT 5: Ionic compounds are/have...
Low melting points
Brittle solids
Gases at room temperature
Weak bonds
30
Neutrons have a negative charge.
True
False
31
Which of the following is a Bronsted-Lowry base?
H3O+
HCl
NH4+
NH3
32
What is the definition of an orbital?
Outermost electrons in the highest energy level of an atom
Sublevels of the main energy shell within an atom
Main energy shells of an atom
Regions in a sublevel where an electron is most likely to be located
33
Fission splits large nuclei
False
True
34
What conversion factor would you use to get from 260 grams to kilograms?
1 kg/100 g
1000 g/1 kg
1 kg/1000 g
100 g/1kg
35
Write the formula for sulfuric acid
H4SO4
HSO4
H2SO2
H2SO4
36
How many moles are in 25.0 grams of water (H₂O)?
1.388 moles
5.899 moles
2.347 moles
4.587 moles
37
How can you balance redox reactions?
Seperate the equation into oxidation and reduction half-reactions
Check the electronegativity of each molecule
Seperate the equation into its spectator ions
Find the molarity of each molecule in a chemical equation
38
Identify the oxidation number from the reaction: Cu^2+ + 2e^- → Cu
4
0
2
1
39
Write the equilibrium constant equation for: CaCO3(s) ⇌ CaO(s) + CO2(g)
[CaCO3] / [CO2]
[CaO] / [CO2]
[CaCO3]
[CO2]
40
Define accuracy in a scientific experiment.
How close a measurement is to the actual value
How many times a scientist gets the exact actual value in an expirement
An independent variable in a scientific expirement
How much time it took to conduct each expirement
41
10 grams of a product was the theoretical yield, but, the actual yield was only 8 grams. What is the percent yield?
92%
80%
75%
85%
42
Emission spectra are produced when electrons become _____ and release light, but then return to lower energy levels.
Energized
Ecstatic
Hyper
Excited
43
How many neutrons are in an atom with a mass number of 27 and an atomic number of 13?
14 neutrons
8 neutrons
10 neutrons
12 neutrons
44
What is the total oxidation number of H2O?
1
3
0
2
45
Protons and neutrons both have a relative mass of:
2 amu
0.5 amu
1.5 amu
1 amu
46
What is the first step to identifying spectator ions in a reaction?
Identifying the state of matter of each molecule
Identifying the relative charge of each molecule
Identifying the electronegativity of each molecule
Identifying the polarity of each molecule
47
Identify the elements and number of atoms in MgCl2
Magnesium and chloride - 5
Magnesium and chloride - 2
Magnesium and chloride - 3
Magnesium and chloride - 1
48
All of the following are examples of things you should do in a lab EXCEPT:
Always washing your hands after labwork
Wearing safety goggles and only take them off when the teacher tells you to
Not eating or drinking while in the labspace
Keeping long hair down when you don't have a hair tie
49
The atomic radius....
Decreases from right to left, increases from bottom to top
Increases from right to left, decreases from bottom to top
Decreases from left to right, increases from top to bottom
Increases from left to right, decreases from top to bottom
50
What is one thing that all balanced nuclear equations have?
The same number of alpha particles on both sides
Same number of neutrons on both sides of the equation
Equal numbers of protons and neutrons in each nucleus
Equal total mass numbers and atomic numbers on both sides of the equation
51
UNIT 6: Covalent molecules are typically _______
Malleable
Brittle
Shiny
Conductive in water
52
If a gas occupies 50.0 liters at STP, how many moles are there?
2.11 mol
2.23 mol
1.79 mol
1. 54 mol
53
Which of the following is a major weakness of Dalton's discoveries?
Had a correct explanation for why isotopes occur
Introduced the concept of atoms
Helped establish a basis for basic chemical reactions/composition
He wrongly stated that atoms are indivisible
54
Find the molarity (M) formula.
M = moles of solute x liter of solution
M = moles of solute / liter of solution
M = moles of solute x liter of solution x 100%
M = liter of solution / moles of solute
55
What is a significant figure?
The digits of a number that is required to express a degree of accuracy
A scientific research method invovling quantative analysis
Another name for a control group in an experiment
Another name for multiplication
56
_______ are generally always soluble
Halogens
Alkali earth metals
Noble gases
Alkali metals
57
A real gas deviates from that of an ideal gas when...
It is at a low pressure
It is at its critical point
It is converting into plasma
It is at a high temperature
58
Alpha particles are the heaviest, but....
They have a moderate amount of ionizing energy
They have the least penetrating power
They have the least ionizing energy
They have a moderate penetrating power
59
Given the example Carbon - 14, what does the "14" in this notation indicate?
Number of protons
Symbol of the element
Mass number
Number of valence electrons
60
What would be considered a successful collision in a chemical reaction?
Collisions with sufficient kinetic energy and correct orientation
Collisions between molecules of the same substance
Collisions with a small amount of kinetic energy
Any collision between molecules
61
What is the pressure of 1.3 moles of a gas in a 20.0 L container at 203 K?
2.02 atm
4.58 atm
1.08 atm
3.76 atm
62
Identify the type of reaction: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Decomposition
Combustion
Neutralization
Single displacement
63
Which acid has the highest Ka value?
HCl
HF
HBrO
HClO4
64
How many grams of NaCl are produced from 2.5 moles of NaCl?
121.07 gams
255.6 grams
395.3 grams
146.1 grams
65
Name the ion: Cl⁻
Chloride (I) ion
Chlorine ion
Chloride ion
Chlorine (I) ion
66
Rank the relative strength of dispersion forces, dipole-dipole, and hydrogen bonding from highest to lowest.
Dipole-dipole, dispersion forces, hydrogen bonding
Dipole-dipole, hydrogen bonding, dispersion forces
Hydrogen bonding, dispersion forces, dipole - dipole
Hydrogen bonding, dipole-dipole, dispersion forces
67
UNIT 8: What is the mole ratio of sodium to chloride in this reaction: 2Na + Cl2 --> 2NaCl?
1:1
1:2
1:4
2:1
68
Which of the following would be the most soluble in water?
An ionic compound
Polar molecule
Nonpolar molecule
A metallic compound
69
An electron in a hydrogen atom transitions from n = 3 level to the n = 2 energy level. Calculate the energy released.
4.245 * 10^-12 J
5.668 * 10^-18 J
3.027 * 10^-19 J
10.992 * 10^-21 J
70
How many orbitals are in an f sublevel?
3
7
5
1
71
If the equilibrium constant is _____, this means the reaction will shift left, favoring the reactants.
The value of K does not matter in this problem
K = 1
K >1
K < 1
72
How many moles of NaCl are in 75 mL of a 0.50 M NaCl solution?
0.11250 moles
0.0375 moles
0.0222 moles
0.4756 moles
73
What is the formula for the formal charge of a Lewis structure?
Formal charge = Valence - Nonbinding electrons - Binding electrons
Formal charge = Valence - Nonbinding electrons - (Binding electrons/2)
Formal charge = Valence + Nonbinding electrons - (Binding electrons/2)
Formal charge = Valence + Nonbinding electrons + Binding electrons
74
Name the acid HClO2
Chlorine acid
Cholric acid
Chlorous acid
Hydrochloric acid
75
According to the kinetic molecular theory of gas, collisions are ______
Elastic
Exothermic
Endothermic
Unchanging
76
Find the answer: (7.5 * 10^3) - (2.1 * 10^5)
-200002
-202500
202555
-200000
77
A reaction has a percent yield of 58% and the theoretical yield is 65 grams. What is the actual yield?
40.8 grams
37.7 grams
50.3 grams
22.5 grams
78
Which of the following defines the mole in chemistry?
A mole represents 6.022 * 10^23 particles (Avogadro's number)
A mole is the mass of one atom of an element measured in grams
A mole is the number of protons and neutrons in the nucleus of an atom
A mole is the mass of one atom of an element measured in kilograms
79
What is the STP of temperature?
1 Celsius
100 K
100 Celsius
273.15 K
80
Rank the following compounds in order of increasing lattice energy: NaCl, MgO, CaO
NaCl, CaO, MgO
NaCl, MgO, CaO
MgO, CaO, NaCl
CaO, MgO, NaCl
81
Within each principal energy level, there are sublevels labeled as s, p, d, and f
False
True
82
A 300 mL beaker has a precision of (+) or (-) 5%. What is the absolute precision?
15 mL
28 mL
6 mL
10 mL
83
Determine the empirical formulas for compounds with the percent composition 15.8% carbon and 84.2% sulfur
C2S3
C4S5
CS2
C2S
84
Find the complete ionic equation for a reaction between aqueous KOH and aqueous HCl?
K+ (aq) + H+ (aq) + OH- (aq) + Cl- (aq) -> H2O (l) + K+ (aq) + Cl- (aq)
K+ (aq) + OH- (aq) + H+ (aq) + Cl- (aq) -> K+ (aq) + Cl- (aq) + H2O (l)
H+ (aq) + OH- (aq) -> H2O (l) H+ (aq) + OH- (aq) -> H2O (l)
KOH (aq) + HCl (aq) -> KCl (aq) + H2O (l)
85
An increase in _____ increases the amount of collisions due to particles being squished closer together.
Catalysts
Pressure
Temperature
Volume
86
A reaction will occur between NaCl and silver nitrate AgNO3
False
True
87
Calculate the amount of heat in joules released when 41.3 g water freezes at 0 C
1.25 * 10^5 J
1.38 * 10^4 J
1.30 * 10^6 J
1.45 * 10^5 J
88
UNIT 7: What is the balanced equation between combustion of methane (CH4) with oxygen to form carbon dioxide and water
CH4 + 4O2→ CO2 + 4H2O
CH4 + 2O2→ 4CO2 + 2H2O
CH4 + O2→ CO2 + H2O
CH4 + 2O2→ CO2 + 2H2O
89
The shielding effect is defined as...
Ability of outer electrons to shield inner electrons from nuclear charge
Ability of nucleus to decrease the charge it projects onto the electrons
Ability of electrons to react with another molecule with less electrons
Ability of inner electrons to shield outer electrons from nuclear charge
90
Which subatomic particle(s) are located in the nucleus?
Protons
Protons and electrons
Protons and neutrons
Neutrons
91
UNIT 3: Which of the following types of waves has the shortest wavelength?
Ultraviolet waves
Microwaves
Gamma waves
Radio waves
92
UNIT 11: Convert 103 atm to mmHg (1 atm = 760 mmHg).
65246
78280
67889
75606
93
How many moles of water are in 1.5 x 10^-30 molecules of water?
1.33 x 10^-22
22.9 x 10^-3
0.78 x 10^85
2.49 × 10^-54 mol
94
How many moles of solute are in 300 mL of a 3.75 M solution?
1.052 mol
1.125 mol
1.025 mol
1.250 mol
95
Calculate 2.40 × 3.52 (with the appropriate number of significant figures)
8.67
8.45
8.50
9.00
96
What does a catalyst do in a reaction?
Increases the temperature
Slows down the reaction
Increases the activation energy
Lowers the activation energy
97
Solids have a....
Definite shape only
None of the above
Definite volume only
Definite shape and volume
98
The atomic number on a periodic table can tell you:
The number of electrons in a neutral atom
The average atomic mass of the element
The number of neutrons in the atom
The number of valence electrons in the atom
99
The molar mass of MgSO4 * 7H2O is 238.52 g/mol
True
False
100
UNIT 4: Identify which of the following is a lanthanide.
Samarium
Rubidium
Carbon
Silicon
101
___ are used to indicate molar concentration
Comma
Hyphens
Parantheses
Brackets
102
How many valence electrons does potassium have, considering its noble gas configuration is [Ar] 4s?
4 valence electrons
2 valence electrons
1 valence electron
3 valence electrons
103
What group number are the halogens?
Group 15
Group 18
Group 17
Group 16
104
What unit is used to measure frequency?
Hertz
Oscillation factor
Wavelength
Kilojoules
105
The Aufbau Principle states that...
No more then two electrons may be in one orbital
Electrons must fill lower energy orbitals first
Electrons pair up in an orbital when all other orbitals have one electron
Two electrons in one orbital must have opposite signs
106
What category of elements on the periodic table require a roman numeral in naming?
Non metals
Alkali metals
Halogens
Transition metals
107
Can you turn a solid into a liquid, and a liquid back into a solid (with regards to water)?
True
False
108
When an electron transitions from a ___ energy level to a ____ one, it absorbs a photon of light.
Higher, lower
Low,er lower
Lower, higher
Higher, higher
109
Ionic compounds have a distinct lattice structure.
False
True
110
What is a limiting reactant in an equation?
The reactant that is partially used up in the reaction
The reactant that is completely used up in the reaction
The reactant that has the highest coefficient in the equation
The reactant that allows the reaction to occur
111
Write the electron configuration of sodium (Na).
1s^2 2s^2 2p^6 3s
1s 4s 3p^2 1d
1s 2s 2p^2 p
1s^2 2s^2 2p 1d
112
Rank the relative strengths of single, double, and triple bonds from highest to lowest
Double, triple, single
Triple, double, single
Single, double, triple
Double, single, triple
113
The "d" block on the periodic table is mostly located in the transition metals region.
True
False
114
The reaction will shift left if stress is added to an endothermic reaction.
True
False
115
Cutting up a powdery substance is an example of a physical change.
True
False
116
Define the theoretical yield.
the smallest amount of product that can be formed from a limiting reactant
the biggest amount of product that can be formed from a limiting reactant
the biggest amount of reactant that can be formed from the products
the smallest amount of reactant that can be formed from the products
117
UNIT 2: Which of the following scientists is correctly matched with their discovery?
Bohr: gold foil experiment
Rutherford: plum pudding model of the atom
Democritus: cathode ray tube experiment
Dalton: suggested that all matter is made of atoms, which are indivisible
118
Which of the following formulas correctly lists Planck's energy formula?
E = v/h
E = h/v
E = hv
E = hv + 3
119
Write the noble gas configuration for oxygen (O).
[Ne] 2s^2 p^4
[He] 2s^2 2p^4
[Ne] s^2 p^4
[He] s^2 p^2
120
Which of the following is the order in which the lowest 3 energy orbitals occupy?
1s, 2s, 1p
1s, 1p, 2s
1s, 2s, 2p
1s, 2s, 3s
121
A gas has an amount of 85 mL at 156 K and 2.1 atm. What will the temp be if the gas increases to 97 mL & 3.5 atm?
255 K
297 K
301 K
232 K
122
Convert 2.15 * 10^3 kilograms to milligrams.
2.15 * 10^9 milligrams
2.15* 10^7 milligrams
2.15 * 10^10 milligrams
2.15 * 10^-5 milligrams
123
All of the following statements about density are correct EXCEPT:
Mass is measured in g
Density is measured in g/cm^3
Volume is measured in cm^3
Density is measured in g/cm
124
NaOH is a strong _____ because it completely dissociates into Na+ and OH- ions in water.
Acid
Base
Solute
Solvent
125
Convert 1.5 x 10^4 to standard form
15000
150000
150
1500
126
What is the formula when solving for density (given the numbers for mass and volume)?
d = mv
d = m(2v)
d = m/v
d = v/m
127
Pressure and volume are in a ______ relationship
Joint
Linear
Inverse
Direct
128
Round 324.55 to 2 significant figures
320
325
300
324
129
What is the acronym for diatomic elements?
BRINCLHOF
BRINGCOLHOF
BRINCOLHOF
BRINCLHOVF
130
Non-metals are generally in the gaseous state of matter.
True
False
131
Which of the following VSEPR structures contains two lone pairs?
Bent
Tetrahedral
Linear
Trigonal Planar
132
Carbon-Hydrogen is a polar bond
False
True
133
A 2.0 L container of gas at 15 Celsius and 3 atm pressure is heated to 58 Celsius. What is the new pressure?
3.76 atm
4.01 atm
3.99 atm
3.45 atm
134
What should you do when trying to find the average atomic mass (given two isotopes of an element)?
Multiply each isotope's mass by its abundance in fraction form
Divide each isotope's mass by its abundance in fraction form
Subtract each isotope's mass by its abundance in fraction form
Add each isotope's mass by its abundance in fraction form
135
A cation is a positively charged ion that gains an electron.
True
False
