Which of the following is not true of combustion reactions?

Liquid water is often produced.

What's the difference between a catalyst and a spectator ion?

Spectator ions are listed in the reaction equation

Two objects are attracted to each other. Can you safely say they each have opposite charges?

No, neutral objects can be attracted to charges if polarized

Why do valence electrons require the least IE to remove?

They have the greatest "shielding effect" from inner shells

Why do ionic compounds tend to dissolve well in water?

Polar H2O molecules surround charged ions, dissociating them

What did Avogadro's number originally describe?

The number of Carbon-12 atoms in exactly 12g of Carbon-12.

You heat potassium chlorate in an opened test tube, and seem to end with less solid mass. Why?

Decomposing KClO3 produces O2, which leaves the test tube

Why do ionic compounds generally have higher melting/boiling points than covalent molecules?

Electrostatic bonds are stronger than intermolecular forces

What is always true about polarization, regardless of whether a substance is metal or nonmetal?

An overall neutral object has areas of net (+) or (-) charge, Electrons are not transferred between two objects.

Why is NaCl called "sodium chloride" when PbO is called "lead (II) oxide"?

Pb is a transition metal, so you need to specify its charge., Na has a fixed charge, so it doesn't need to be specified.

What is not true about mixtures?

Every mixture exists in one uniform phase

Why is alcohol better than water for use in a thermometer?

Alcohol's boiling point is lower, so it expands more easily, Alcohol's freezing point is lower, so it won't freeze easily

Can a reaction requiring activation energy still be considered exothermic?

Yes, as long as energy released > activation energy

Iodine-125 has a half-life of 59.49 days. How long will it take for an atom of I-125 to decay?

Decay is actually a random event, half-life is just a trend

Why does a steam-filled soda can implode if you throw it into ice water?

The steam condenses rapidly and creates an empty vacuum

Studying how and why matter interacts with itself or changes, Identifying and classifying substances or reactions, All of the above, Using the properties of substances/matter to create new ones

Why does hydrogen only hold 2 valence electrons at most?

It only has 1 proton, which can't hold together 8 electrons

What is the purpose of significant figures?

They indicate the degree of uncertainty of your measurements

How does positron emission affect the mass of an atom?

It doesn't, as protons and neutrons have the same mass.

Would hydrochloric acid be considered an ionic compound?

No, it's a polar covalent compound (0.4 < ΔEN < 2.0)

If you stack 2 conductive cans and place a (-) balloon next to can 1, how do the (e-) move?

(e-) move from Can 1 to Can 2, as the cans form one system

What did Rutherford's gold foil experiment prove?

Atoms had a lot of empty space, and a positive core

Balance this equation: C3H8 reacts with oxygen to form carbon dioxide and water.

C3H8 (g) + 5O2 (g) -> 4H2O (g) + 3CO2 (g)

Why is simple distillation able to separate a mixture of two liquids?

One liquid evaporates away due to a lower boiling point

Why can a mix of alcohol/water RE-light a match, even though the mix can't produce open flames?

Separated alcohol vapor re-ignites the match.

What is the relationship between an element's molar mass (g/mol) and atomic mass (a.m.u)?

They're the same number, just with different units.

What might cause a percent yield greater than 100%?

Contamination of the final product

Why does the octet rule take precedence over Mendeleev's "valence" measurements of hydrides?

Valence power only explains hydrides, not other compounds.

How do ionic and covalent bonds differ?

Ionic bonds can never be polar, but covalent bonds can., In covalent bonds, electrons are shared, not transferred.

What is not true of double-replacement reactions?

The reactivity series is used to determine if it will occur

studbud

Honors Chem 2018-2019 review

57 termsStudBud Administration20 plays

Review of the material covered in honors chem 2019-2019, units 1-7. Note that due to Quiz's character limits, the questions and answers aren't as in-depth as I'd have liked. Still, if anything needs fixing (I make mistakes too) let me know ASAP. Good luck on the finals!

Flashcards57 cardsFPractice quizPHost liveL

Questions 57

Answers

1
Which of the following is not true of combustion reactions?
Oxides are produced from the reaction.
Liquid water is often produced.
They generally release energy in the forms of light/heat.
Hydrocarbons are reacted with oxygen.
2
What's the difference between a catalyst and a spectator ion?
Spectator ions are actually involved in electron transfer
A spectator ion must be monatomic, a catalyst is polyatomic.
Spectator ions are listed in the reaction equation
A catalyst is changed in the reaction, but a spectator isn't
3
Two objects are attracted to each other. Can you safely say they each have opposite charges?
Yes, because opposite charges attract
No, neutral objects can be attracted to charges if polarized
Yes, since if the objects were neutral, nothing would happen
No, there could be unknown forces pushing them together
4
Why do valence electrons require the least IE to remove?
Because they're the electrons involved in chemical reactions
They're found on the surface of the atom
They have the greatest "shielding effect" from inner shells
Valence shells can hold up to 8 electrons, which is unstable
5
You react 127.10g Cu with 679.48g Ag(NO3) and get 337.61g of Cu(NO3)2. What's your % yield?
85%
80%
90%
92.5%
6
Why do ionic compounds tend to dissolve well in water?
Because water is the universal solvent
Polar H2O molecules surround charged ions, dissociating them
The ions can bond with the water molecules, forming hydrates
Ionic bonds are polar like water, and likes dissolve likes.
7
What did Avogadro's number originally describe?
The charge of an electron (in coulombs).
The temperature (K°) at which all particle movement ceases.
The number of Carbon-12 atoms in exactly 12g of Carbon-12.
The max distance that the strong force is effective (in nm)
8
Th-232 undergoes alpha decay, and its product undergoes beta decay. What's the final isotope?
Actinium-228
Thorium-228
Radon-228
Protactinium-229
9
You heat potassium chlorate in an opened test tube, and seem to end with less solid mass. Why?
Decomposing KClO3 produces O2, which leaves the test tube
Trick question - mass is always conserved in a reaction
Decomposing KClO3 produces Cl2, which leaves the test tube
Heating KClO3 reacts it with oxygen, so you lose some KClO3
10
Why is a balanced chemical equation helpful?
You can use it to calculate limiting reagents
It tells you the stoichiometric ratio of a reaction
You can use it to calculate theoretical yield
All of the above
11
Why do ionic compounds generally have higher melting/boiling points than covalent molecules?
Electrostatic bonds are stronger than intermolecular forces
Metals in ionic compounds hold electrons much more tightly
An ionic bond is polar, so it takes more energy to break
Because covalent molecules can only form 1, 2, or 3 bonds.
12
What is always true about polarization, regardless of whether a substance is metal or nonmetal?
Non-metals tend to become more polarized than metals.
Electrons can't move between atoms, only within their atoms.
An overall neutral object has areas of net (+) or (-) charge
Electrons are not transferred between two objects.
13
What are some known limitations of the Bohr model?
All are correct
It does not account for sub-orbitals or different types
Orbitals aren't truly fixed, just the most likely positions
It was only ever used accurately with hydrogen.
14
Why is NaCl called "sodium chloride" when PbO is called "lead (II) oxide"?
the (II) in PbO means that it has a 2- charge.
Pb is a transition metal, so you need to specify its charge.
PbO is covalent, and covalent compounds have no charges.
Na has a fixed charge, so it doesn't need to be specified.
15
What is not true about mixtures?
They can be separated by a physical method (i.e filtration)
None of these are incorrect.
Elements in a mixture retain their characteristic properties
Every mixture exists in one uniform phase
16
Why is alcohol better than water for use in a thermometer?
Water's boiling point is lower, so it expands more easily
H2O's freezing point is higher (easy to tell when it's 32F)
Alcohol's boiling point is lower, so it expands more easily
Alcohol's freezing point is lower, so it won't freeze easily
17
If in a mole of H2O there are 2 moles of H atoms and one mole of O atoms, what else is true?
All of the above
In 10 molecules of H2O, there are 20 H atoms and 10 O atoms
In 2 mol H2O, there are 4 mol H atoms and 2 mol O atoms
In one molecule of H2O, there are 2 H atoms and 1 O atom
18
Can a reaction requiring activation energy still be considered exothermic?
No, the activation energy stays stored in new chemical bonds
Yes, if the temperature of the product(s) drops afterwards.
No, reactions that absorb energy are always endothermic.
Yes, as long as energy released > activation energy
19
Iodine-125 has a half-life of 59.49 days. How long will it take for an atom of I-125 to decay?
59.49 days
118.98 days
Decay is actually a random event, half-life is just a trend
We'd need the half-lives of other iodine isotopes to tell
20
Which of the following substances cannot be represented at the particle level?
Elements
Compounds
Heterogeneous solutions
Homogeneous solutions
21
What do nuclear and chemical reactions have in common?
Neutron count changes nuclear properties, not chemical
A chemical rxn can't affect the nucleus, a nuclear rxn does
They both produce very large amounts of energy.
None of these are correct
22
Why does IE increase as you move down a period, but decrease as you move down a group?
Moving across in a period adds protons (Z effect)
Moving across a period adds electrons, but no shielding
Moving down a group adds extra orbitals (more shielding)
All of the above
23
Why does a steam-filled soda can implode if you throw it into ice water?
The can is unable to withstand sudden temperature changes
The steam condenses rapidly and creates an empty vacuum
Steam is displaced by water, and water is more dense
The ice is packed tightly enough to crush the can
24
What is chemistry?
Studying how and why matter interacts with itself or changes
Identifying and classifying substances or reactions
All of the above
Using the properties of substances/matter to create new ones
25
Which number has five significant figures?
10.000
1000.
10,000
100.0
26
Why does hydrogen only hold 2 valence electrons at most?
It only has 1 proton, which can't hold together 8 electrons
Because it's the lightest element
Because most hydrogen isotopes have 2 neutrons
So it can easily form single bonds with other atoms
27
You react 130.78g of Zn with 106.35g of Cl2. What is left over from this reaction?
65.39g of leftover zinc
35.45g of leftover chlorine
32.70g of leftover chlorine
32.70g of leftover zinc
28
What is the purpose of significant figures?
To punish students who fail to round carefully
Rounding makes calculations/following work easier.
They measure the level of precision that you chose to use
They indicate the degree of uncertainty of your measurements
29
How does positron emission affect the mass of an atom?
It doesn't, as protons and neutrons have the same mass.
The loss of a proton decreases the mass number by 1.
The gain of a neutron increases the mass number by 1.
It doesn't; positrons are emitted due to alpha radiation.
30
Why was James Chadwick's discovery of the neutron significant?
It helped explain why protons don't repel in the nucleus
It fixed discrepancies between atomic mass and atomic number
Every answer is correct
Neutrons gave an explanation for the existence of isotopes
31
Would hydrochloric acid be considered an ionic compound?
No, as it's two nonmetals bonded together.
Yes, as it dissociates in water and forms ions
No, it's a polar covalent compound (0.4 < ΔEN < 2.0)
Yes, as even though hydrogen is a nonmetal, it acts like one
32
List all of the diatomic elements.
Hg, N, F, O, I, Cl, Br
He, F, O, I, Cl, Br, Xe
H, N, F, O, I, Cl, Br
H, F, O, I, Cl, Br, At
33
What isn't needed to prove that 2 containers of gas have the same number of gas molecules?
Mass
Pressure
Volume
Temperature
34
If you stack 2 conductive cans and place a (-) balloon next to can 1, how do the (e-) move?
(e-) stay in Can 1, and move within their original atoms
(e-) move from Can 1 to Can 2, as the cans form one system
(e-) stay in Can 1, but move between atoms to the edge of it
The balloon will touch Can 1 and pop
35
What is the charge of a cadmium ion?
Fixed 2+ charge
It's a transition metal, so it has a variable charge
Cadmium is a special case that doesn't form ions
Fixed 1+ charge
36
You fully react 190.65g of Cu with AgNO3; you get 562.68g of Cu(NO3)2. How much AgNO3 was used?
509.61g AgNO3
372.03g AgNO3
849.35g AgNO3
1019.28g AgNO3
37
Ag's average mass is ~107.9g; find its 2 isotopes. One of them is Ag-107 (51.86% abundance).
Ag-110
Ag-108
Ag-111
Ag-109
38
What did Rutherford's gold foil experiment prove?
Every answer is right
Electrons had very little mass relative to protons
Electrons orbited the surface of the atom in fixed positions
Atoms had a lot of empty space, and a positive core
39
Which measurement is equal to 1,000 cubic centimeters?
10 milliliters
1 liter
0.01 cubic meters
0.1 cubic meters
40
Balance this equation: C3H8 reacts with oxygen to form carbon dioxide and water.
C3H8 (g) + 5O2 (g) -> 4H2O (l) + 3CO2 (g)
C3H8(g) + 10 O(g) -> 4H2O(g) + 3CO2 (g)
0.5 C3H8 (g) + 2.5 O2 (g) -> 2H2O (l) + 1.5 CO2 (g)
C3H8 (g) + 5O2 (g) -> 4H2O (g) + 3CO2 (g)
41
You dissolve 12.97g of LiF in water to get an 0.87M LiF solution. What's the solution's volume?
11.4 liters
14.5 liters
14.7 liters
0.57 liters
42
You mix 45.98g of sodium with 106.35g of elemental chlorine. How much NaCl is produced?
87.66g
146.1g
116.88g
58.44g
43
Why is simple distillation able to separate a mixture of two liquids?
The cooler liquid at the top ends up settling to the bottom.
The liquid at the bottom becomes hotter and rises to the top
The heat breaks chemical bonds and separates the two liquids
One liquid evaporates away due to a lower boiling point
44
Why can a mix of alcohol/water RE-light a match, even though the mix can't produce open flames?
The mixture releases H2 gas, which is flammable.
Trick question: this mixture can't reignite a match.
Separated alcohol vapor re-ignites the match.
The mixture releases O2 gas, which is flammable.
45
Which of the following are considered pure substances?
Both elements and compounds
Compounds
Elements
Mixtures of elements
46
What is the relationship between an element's molar mass (g/mol) and atomic mass (a.m.u)?
You can convert g/mol to amu if you multiply by 1.6 x 10^-19
We can easily use them both to determine empirical formulas
They're the same number, just with different units.
Neither molar or atomic mass are relative mass measurements.
47
What might cause a percent yield greater than 100%?
Losing some product and failing to account for it
Failing to fully use all of the reactants
Contamination of the final product
Losing some reactant and failing to account for it
48
Why does the octet rule take precedence over Mendeleev's "valence" measurements of hydrides?
Valence power only explains hydrides, not other compounds.
Valence power doesn't tell you how two atoms will bond.
All of the above
There were too many exceptions in the valence power rules.
49
How do ionic and covalent bonds differ?
Ionic bonds can never be polar, but covalent bonds can.
Ionic substances are usually liquid at room temperature.
In covalent bonds, electrons are shared, not transferred.
Covalent bonds are more likely to be soluble in water.
50
You have 302.2 kg of 500. m solution, containing 292.2 kg of dissolved solute. Find the solute.
NaCl
BeF2
MgO
Al2O3
51
What is not true of double-replacement reactions?
One product will be either a gas or a solid precipitate
One product will be an aqueous solution
The reactivity series is used to determine if it will occur
Both reactants are usually aqueous
52
What term describes two atoms with identical electron configurations?
Isoelectric
Isoelectronic
Isoionic
Isonuclear
53
Why is neutral tinfoil more polarized than neutral paper in the presence of a charged object?
Foil is a better insulator, so its e- move between atoms
Actually, neither of them become polarized (no e- transfer)
Paper is a better insulator, so its e- move between atoms
Foil is a better conductor, so its e- move between atoms
54
Why are the mole and its applications helpful?
Mole ratios are directly proportional to atom ratios.
Molar masses close the gap between the micro and macroscopic
We can't work with individual atoms, but we can use moles.
Every answer is correct
55
Are there any similarities between atomic size trends and electronegativity trends?
They're not related.
As atoms grow smaller, they become less electronegative.
As atoms grow larger, they become more electronegative.
As atoms grow smaller, they become more electronegative.
56
You ignite Mg with a match, producing blinding light and heat. Do you write Δ over the arrow?
No, because some energy was still released.
Yes, as you had to add energy to start the reaction.
Yes, since this reaction is endothermic.
No, as you didn't need to add energy continuously.
57
In covalent bonds, why do halogens usually only form single bonds?
Halogens have an odd # of valence electrons.
Halogens are the most electronegative group.
They all have 7 valence (e-), so they can only take one (e-)
Forming a double bond leaves an odd number of valence (e-)

Honors Chem 2018-2019 review Flashcards | StudBud

Honors Chem 2018-2019 review

57 termsStudBud Administration20 plays

Flashcards57 cardsFPractice quizPHost liveL

Questions 57

Answers

1
Which of the following is not true of combustion reactions?
Oxides are produced from the reaction.
Liquid water is often produced.
They generally release energy in the forms of light/heat.
Hydrocarbons are reacted with oxygen.
2
What's the difference between a catalyst and a spectator ion?
Spectator ions are actually involved in electron transfer
A spectator ion must be monatomic, a catalyst is polyatomic.
Spectator ions are listed in the reaction equation
A catalyst is changed in the reaction, but a spectator isn't
3
Two objects are attracted to each other. Can you safely say they each have opposite charges?
Yes, because opposite charges attract
No, neutral objects can be attracted to charges if polarized
Yes, since if the objects were neutral, nothing would happen
No, there could be unknown forces pushing them together
4
Why do valence electrons require the least IE to remove?
Because they're the electrons involved in chemical reactions
They're found on the surface of the atom
They have the greatest "shielding effect" from inner shells
Valence shells can hold up to 8 electrons, which is unstable
5
You react 127.10g Cu with 679.48g Ag(NO3) and get 337.61g of Cu(NO3)2. What's your % yield?
85%
80%
90%
92.5%
6
Why do ionic compounds tend to dissolve well in water?
Because water is the universal solvent
Polar H2O molecules surround charged ions, dissociating them
The ions can bond with the water molecules, forming hydrates
Ionic bonds are polar like water, and likes dissolve likes.
7
What did Avogadro's number originally describe?
The charge of an electron (in coulombs).
The temperature (K°) at which all particle movement ceases.
The number of Carbon-12 atoms in exactly 12g of Carbon-12.
The max distance that the strong force is effective (in nm)
8
Th-232 undergoes alpha decay, and its product undergoes beta decay. What's the final isotope?
Actinium-228
Thorium-228
Radon-228
Protactinium-229
9
You heat potassium chlorate in an opened test tube, and seem to end with less solid mass. Why?
Decomposing KClO3 produces O2, which leaves the test tube
Trick question - mass is always conserved in a reaction
Decomposing KClO3 produces Cl2, which leaves the test tube
Heating KClO3 reacts it with oxygen, so you lose some KClO3
10
Why is a balanced chemical equation helpful?
You can use it to calculate limiting reagents
It tells you the stoichiometric ratio of a reaction
You can use it to calculate theoretical yield
All of the above
11
Why do ionic compounds generally have higher melting/boiling points than covalent molecules?
Electrostatic bonds are stronger than intermolecular forces
Metals in ionic compounds hold electrons much more tightly
An ionic bond is polar, so it takes more energy to break
Because covalent molecules can only form 1, 2, or 3 bonds.
12
What is always true about polarization, regardless of whether a substance is metal or nonmetal?
Non-metals tend to become more polarized than metals.
Electrons can't move between atoms, only within their atoms.
An overall neutral object has areas of net (+) or (-) charge
Electrons are not transferred between two objects.
13
What are some known limitations of the Bohr model?
All are correct
It does not account for sub-orbitals or different types
Orbitals aren't truly fixed, just the most likely positions
It was only ever used accurately with hydrogen.
14
Why is NaCl called "sodium chloride" when PbO is called "lead (II) oxide"?
the (II) in PbO means that it has a 2- charge.
Pb is a transition metal, so you need to specify its charge.
PbO is covalent, and covalent compounds have no charges.
Na has a fixed charge, so it doesn't need to be specified.
15
What is not true about mixtures?
They can be separated by a physical method (i.e filtration)
None of these are incorrect.
Elements in a mixture retain their characteristic properties
Every mixture exists in one uniform phase
16
Why is alcohol better than water for use in a thermometer?
Water's boiling point is lower, so it expands more easily
H2O's freezing point is higher (easy to tell when it's 32F)
Alcohol's boiling point is lower, so it expands more easily
Alcohol's freezing point is lower, so it won't freeze easily
17
If in a mole of H2O there are 2 moles of H atoms and one mole of O atoms, what else is true?
All of the above
In 10 molecules of H2O, there are 20 H atoms and 10 O atoms
In 2 mol H2O, there are 4 mol H atoms and 2 mol O atoms
In one molecule of H2O, there are 2 H atoms and 1 O atom
18
Can a reaction requiring activation energy still be considered exothermic?
No, the activation energy stays stored in new chemical bonds
Yes, if the temperature of the product(s) drops afterwards.
No, reactions that absorb energy are always endothermic.
Yes, as long as energy released > activation energy
19
Iodine-125 has a half-life of 59.49 days. How long will it take for an atom of I-125 to decay?
59.49 days
118.98 days
Decay is actually a random event, half-life is just a trend
We'd need the half-lives of other iodine isotopes to tell
20
Which of the following substances cannot be represented at the particle level?
Elements
Compounds
Heterogeneous solutions
Homogeneous solutions
21
What do nuclear and chemical reactions have in common?
Neutron count changes nuclear properties, not chemical
A chemical rxn can't affect the nucleus, a nuclear rxn does
They both produce very large amounts of energy.
None of these are correct
22
Why does IE increase as you move down a period, but decrease as you move down a group?
Moving across in a period adds protons (Z effect)
Moving across a period adds electrons, but no shielding
Moving down a group adds extra orbitals (more shielding)
All of the above
23
Why does a steam-filled soda can implode if you throw it into ice water?
The can is unable to withstand sudden temperature changes
The steam condenses rapidly and creates an empty vacuum
Steam is displaced by water, and water is more dense
The ice is packed tightly enough to crush the can
24
What is chemistry?
Studying how and why matter interacts with itself or changes
Identifying and classifying substances or reactions
All of the above
Using the properties of substances/matter to create new ones
25
Which number has five significant figures?
10.000
1000.
10,000
100.0
26
Why does hydrogen only hold 2 valence electrons at most?
It only has 1 proton, which can't hold together 8 electrons
Because it's the lightest element
Because most hydrogen isotopes have 2 neutrons
So it can easily form single bonds with other atoms
27
You react 130.78g of Zn with 106.35g of Cl2. What is left over from this reaction?
65.39g of leftover zinc
35.45g of leftover chlorine
32.70g of leftover chlorine
32.70g of leftover zinc
28
What is the purpose of significant figures?
To punish students who fail to round carefully
Rounding makes calculations/following work easier.
They measure the level of precision that you chose to use
They indicate the degree of uncertainty of your measurements
29
How does positron emission affect the mass of an atom?
It doesn't, as protons and neutrons have the same mass.
The loss of a proton decreases the mass number by 1.
The gain of a neutron increases the mass number by 1.
It doesn't; positrons are emitted due to alpha radiation.
30
Why was James Chadwick's discovery of the neutron significant?
It helped explain why protons don't repel in the nucleus
It fixed discrepancies between atomic mass and atomic number
Every answer is correct
Neutrons gave an explanation for the existence of isotopes
31
Would hydrochloric acid be considered an ionic compound?
No, as it's two nonmetals bonded together.
Yes, as it dissociates in water and forms ions
No, it's a polar covalent compound (0.4 < ΔEN < 2.0)
Yes, as even though hydrogen is a nonmetal, it acts like one
32
List all of the diatomic elements.
Hg, N, F, O, I, Cl, Br
He, F, O, I, Cl, Br, Xe
H, N, F, O, I, Cl, Br
H, F, O, I, Cl, Br, At
33
What isn't needed to prove that 2 containers of gas have the same number of gas molecules?
Mass
Pressure
Volume
Temperature
34
If you stack 2 conductive cans and place a (-) balloon next to can 1, how do the (e-) move?
(e-) stay in Can 1, and move within their original atoms
(e-) move from Can 1 to Can 2, as the cans form one system
(e-) stay in Can 1, but move between atoms to the edge of it
The balloon will touch Can 1 and pop
35
What is the charge of a cadmium ion?
Fixed 2+ charge
It's a transition metal, so it has a variable charge
Cadmium is a special case that doesn't form ions
Fixed 1+ charge
36
You fully react 190.65g of Cu with AgNO3; you get 562.68g of Cu(NO3)2. How much AgNO3 was used?
509.61g AgNO3
372.03g AgNO3
849.35g AgNO3
1019.28g AgNO3
37
Ag's average mass is ~107.9g; find its 2 isotopes. One of them is Ag-107 (51.86% abundance).
Ag-110
Ag-108
Ag-111
Ag-109
38
What did Rutherford's gold foil experiment prove?
Every answer is right
Electrons had very little mass relative to protons
Electrons orbited the surface of the atom in fixed positions
Atoms had a lot of empty space, and a positive core
39
Which measurement is equal to 1,000 cubic centimeters?
10 milliliters
1 liter
0.01 cubic meters
0.1 cubic meters
40
Balance this equation: C3H8 reacts with oxygen to form carbon dioxide and water.
C3H8 (g) + 5O2 (g) -> 4H2O (l) + 3CO2 (g)
C3H8(g) + 10 O(g) -> 4H2O(g) + 3CO2 (g)
0.5 C3H8 (g) + 2.5 O2 (g) -> 2H2O (l) + 1.5 CO2 (g)
C3H8 (g) + 5O2 (g) -> 4H2O (g) + 3CO2 (g)
41
You dissolve 12.97g of LiF in water to get an 0.87M LiF solution. What's the solution's volume?
11.4 liters
14.5 liters
14.7 liters
0.57 liters
42
You mix 45.98g of sodium with 106.35g of elemental chlorine. How much NaCl is produced?
87.66g
146.1g
116.88g
58.44g
43
Why is simple distillation able to separate a mixture of two liquids?
The cooler liquid at the top ends up settling to the bottom.
The liquid at the bottom becomes hotter and rises to the top
The heat breaks chemical bonds and separates the two liquids
One liquid evaporates away due to a lower boiling point
44
Why can a mix of alcohol/water RE-light a match, even though the mix can't produce open flames?
The mixture releases H2 gas, which is flammable.
Trick question: this mixture can't reignite a match.
Separated alcohol vapor re-ignites the match.
The mixture releases O2 gas, which is flammable.
45
Which of the following are considered pure substances?
Both elements and compounds
Compounds
Elements
Mixtures of elements
46
What is the relationship between an element's molar mass (g/mol) and atomic mass (a.m.u)?
You can convert g/mol to amu if you multiply by 1.6 x 10^-19
We can easily use them both to determine empirical formulas
They're the same number, just with different units.
Neither molar or atomic mass are relative mass measurements.
47
What might cause a percent yield greater than 100%?
Losing some product and failing to account for it
Failing to fully use all of the reactants
Contamination of the final product
Losing some reactant and failing to account for it
48
Why does the octet rule take precedence over Mendeleev's "valence" measurements of hydrides?
Valence power only explains hydrides, not other compounds.
Valence power doesn't tell you how two atoms will bond.
All of the above
There were too many exceptions in the valence power rules.
49
How do ionic and covalent bonds differ?
Ionic bonds can never be polar, but covalent bonds can.
Ionic substances are usually liquid at room temperature.
In covalent bonds, electrons are shared, not transferred.
Covalent bonds are more likely to be soluble in water.
50
You have 302.2 kg of 500. m solution, containing 292.2 kg of dissolved solute. Find the solute.
NaCl
BeF2
MgO
Al2O3
51
What is not true of double-replacement reactions?
One product will be either a gas or a solid precipitate
One product will be an aqueous solution
The reactivity series is used to determine if it will occur
Both reactants are usually aqueous
52
What term describes two atoms with identical electron configurations?
Isoelectric
Isoelectronic
Isoionic
Isonuclear
53
Why is neutral tinfoil more polarized than neutral paper in the presence of a charged object?
Foil is a better insulator, so its e- move between atoms
Actually, neither of them become polarized (no e- transfer)
Paper is a better insulator, so its e- move between atoms
Foil is a better conductor, so its e- move between atoms
54
Why are the mole and its applications helpful?
Mole ratios are directly proportional to atom ratios.
Molar masses close the gap between the micro and macroscopic
We can't work with individual atoms, but we can use moles.
Every answer is correct
55
Are there any similarities between atomic size trends and electronegativity trends?
They're not related.
As atoms grow smaller, they become less electronegative.
As atoms grow larger, they become more electronegative.
As atoms grow smaller, they become more electronegative.
56
You ignite Mg with a match, producing blinding light and heat. Do you write Δ over the arrow?
No, because some energy was still released.
Yes, as you had to add energy to start the reaction.
Yes, since this reaction is endothermic.
No, as you didn't need to add energy continuously.
57
In covalent bonds, why do halogens usually only form single bonds?
Halogens have an odd # of valence electrons.
Halogens are the most electronegative group.
They all have 7 valence (e-), so they can only take one (e-)
Forming a double bond leaves an odd number of valence (e-)