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Ch 2 Review (1.1 + 1.2)

Total questions: 142

Worksheet time: 2hrs 36mins

Name
Class
Date
1.
Which type of model is shown?
a)
Plum Pudding
b)
Bohr / Orbits
c)
Electron Cloud
d)
Billiard Ball
2.

Which subatomic particle is not located in the nucleus of the atom?

a)

proton

b)

neutron

c)

electron

d)

none of the above

3.
Which letter represents an electron?
a)
A
b)
B
c)
C
d)
D
4.
Can an atom of Hydrogen have 2 protons?
a)
Yes, because it can be an ion
b)
No, because protons identify the atom
c)
Yes, because it can be an isotope
d)
No, because only neutral atoms exist
5.

Selena performs an experiment to determine if air is made of matter. She takes the mass of a syringe that is vacuum sealed and then re-takes the mass of the syringe when the vacuum seal is broken. Below are her results. What can she conclude from her experiment?

a)

Yes, air is matter because it has both volume and mass

b)

No, air is not matter it only has volume but no mass

c)

No, air is not matter it only has mass but no volume

d)

Yes, air is matter because it has either mass or volume

6.

If the mass number of this chlorine atom is 36, how many neutrons does it have?

a)

17

b)

18

c)

19

d)

can't be determined

7.
The positively charged particles of an atom are the ________.
a)
electrons
b)
protons
c)
neutrons
d)
protons & neutrons
8.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
9.

All matter is made of _________.

a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
10.

What did Bohr’s experiments tell us about the atom?

a)

Bohr discovered that atoms existed

b)

Bohr discovered that electrons orbit the nucleus

c)

Bohr discovered electrons existed

d)

Bohr discovered atoms were 99.99% empty space

11.

What does the atomic number tell us?

a)

How many electrons an element has

b)

How many neutrons an element has

c)

How many protons an element has

d)

How many protons and neutrons an element has

12.

Which of the following is unique for any given element?

a)

the number of neutrons

b)

the charge on the electrons

c)

the number of protons

d)

the mass of a neutron

13.

Which statement about subatomic particles is NOT true?

a)

Protons and Neutrons have almost the same mass

b)

Protons and Electrons have opposite charges

c)

Unlike Protons and Electrons, Neutrons have no charge

d)

Protons and Neutrons have the same charge

14.

The number of protons in one atom of an element is that element's

a)

mass number

b)

isotope

c)

atomic number

d)

balanced charge

15.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost energy level of an atom

16.

Hydrogen Bonds typically occur between atoms of hydrogen involved in this type of bond:

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Nonpolar AND Polar Covalent

17.

TRUE OR FALSE:

Hydrogen bonds are very strong interactions between two atoms.

a)

True

b)

False

18.

The Oxygen atoms in the molecule shown have this charge:

a)

Positive

b)

Partial Positive

c)

Negative

d)

Partial Negative

19.

The Hydrogen atoms in the molecule shown have this charge:

a)

Positive

b)

Partial Positive

c)

Negative

d)

Partial Negative

20.

Which type of chemical bond is formed when electrons are shared and is a stronger bond that is not easily broken?

a)

Ionic bond

b)

Covalent bond

c)

Hydrogen bond

d)

Van der Waals force

21.

Which type of water property explains water's ability to stick to other material.

a)

Cohesion

b)

Surface tension

c)

Adhesion

d)

High specific heat

22.

A material is hydrophobic, that means it...

a)

Doesn't mix with water or dissolve in water easily

b)

Mixes with water or dissolves in water easily

23.

Evaporative cooling

a)

Cools down an animal's body

b)

Cools down the environment

c)

Cools down both an animal's body and the environment

24.

Water is...

a)

Polar

b)

Nonpolar

25.
What makes a molecule polar?
a)
Equal sharing of valence electrons
b)
Unequal sharing of valence electrons
c)
Stealing of electrons
d)
Temporary charges that come and go
26.
Water molecules require a lot of energy to break the hydrogen bonds.  This gives water a high
a)
density
b)
polarity
c)
solvency
d)
specific heat
27.
Because water has a positively charged end and a negatively charged end, it can be described as
a)
amphipathic
b)
hydrophobic
c)
polar
d)
nonpolar
28.
Which of the following properties of water enables molecules to cling together as they move from the roots to the leaves of plants?
a)
Water expands as it freezes.
b)
Water is an excellent solvent.
c)
Water exhibits cohesive behavior.
d)
Water moderates temperature.
29.
Large bodies of water do not quickly fluctuate, or change, in temperature. Why?
a)
Water is a solvent.
b)
Water has a high heat capacity.
c)
Water acts as a buffer.
d)
Water is non-polar.
30.
Some insects can stand on the surface of calm water. Their feet push the surface of the water down slightly, but they do not break the surface. Why?
a)
The insects are light enough so they do not break the hydrogen bonds holding the water molecules together
b)
The insects actually use their wings to hover slightly above the water’s surface and they only skim it with their feet.
c)
The insect’s feet are non-polar, so they are repelled by the polar water molecules and are pushed away from the water’s surface.
d)
The insects are small enough to see the individual water molecules, so they are able to step carefully from one molecule to the next
31.
Why does water move from the roots to the leaves of plants?
a)
Water is pushed by solutes.
b)
Capillary action pulls the water molecules like a chain.
c)
Water is pulled by gravity.
d)
Water’s cohesion causes it to “pull” towards the leaves.
32.
Why does ice float?
a)
As water freezes, it expands and its density decreases.
b)
As water freezes, it takes up more hydrogen from the atmosphere, causing it to have a greater buoyancy.
c)
As water freezes, air becomes trapped between the hydrogen bonds of water molecules.
d)
As water freezes, it takes up more oxygen from the atmosphere, causing it to have a greater buoyancy.
33.
What property of water helps to moderate earth's temperature?
a)
adhesion
b)
chohesion
c)
Specific heat capacity
d)
Latent heat of vaporization
34.
Which of the following is correctly defined as the attraction of the hydrogen from one molecule to the oxygen of a different molecule?
a)
amphipathic
b)
hydrophobic
c)
hydrogen bonding
d)
adhesion
35.
The fact that ice floats on liquid water is due to the fact that water's solid is ___________ than it's liquid form
a)
less polar
b)
more polar
c)
less dense
d)
more dense
36.
The property of water that allows water molecules to stick to another substance is
a)
adhesion
b)
cohesion
c)
density
d)
specific heat
37.
The property of water that allows water molecules to stick to each other is
a)
adhesion
b)
cohesion
c)
density
d)
specific heat
38.
 Many fish and aquatic plants can survive a cold winter because the layer of ice that forms at the top of the lake insulates the water below and prevents the lake from freezing solid. What unique property of water contributes to this effect? 
a)
Water absorbs heat when it evaporates and forms a gas 
b)
 Water expands and becomes less dense when it freezes.
c)
Water molecules completely separate into ions in solutions.
d)
 Water forms hydrogen bonds with ions and other polar substances. 
39.
Water makes up approximately 60% of the human body and plays a vital role in regulating body temperature. Which property of water makes it good at regulating temperature?
a)
Water is a good solvent.
b)
Water exhibits strong cohesion.
c)
. Water has an unusual crystalline structure.
d)
Water has a high capacity for heat.
40.
A florist places a bouquet of white carnations in water containing blue dye. After a time, the flowers turn blue. What process helped the carnations to change color?
a)
Specific heat 
b)
Surface tension
c)
Cohesion and adhesion of water molecules 
d)
Formation of covalent bonds between hydrogen and oxygen molecules
41.
 Small insects can walk across the surface of calm water. Their feet push the surface of the water down slightly, somewhat like a person walking across a trampoline, but they do not break the surface. What is the best explanation for why this happens?
a)
The insects are light enough so that they do not break the hydrogen bonds holding the water molecules together
b)
The insects actually use their wings to hover slightly above the water's surface and they only skim it with their feet
c)
The insects' feet are non-polar, so they are repelled by the polar water molecules and are pushed away from the water's surface
d)
The insects are small enough to see the individual water molecules, so they are able to step carefully from one molecule to the next
42.
What makes a molecule polar?
a)
Equal sharing of valence electrons
b)
Unequal sharing of valence electrons
c)
Stealing of electrons
d)
Temporary charges that come and go
43.

Water is an excellent solvent. Select the property that justifies this statement.

a)

as a polar molecule, it can surround and dissolve ionic and polar molecules

b)

it forms ionic bonds with ions, hydrogen bonds with polar molecules, and hydrophobic interactions with non polar molecules

c)

it forms hydrogen bonds with itself so cohesion is possible

d)

it is liquid and will adhere to many substances

44.

The partial negative charge at one end of a water molecule is attracted to a partial positive charge of another water molecule. What is this type of attraction called?

a)

a polar covalent bond

b)

an ionic bond

c)

a hydration shell

d)

a hydrogen bond

45.

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by

a)

hydrogen bonds.

b)

nonpolar covalent bonds

c)

polar covalent bonds.

d)

ionic bonds.

e)

van der Waals interactions

46.

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called?

a)

a covalent bond

b)

a hydrogen bond

c)

an ionic bond

d)

a hydrophilic bond

e)

a hydrophobic bond

47.

An example of a hydrogen bond is the bond between

a)

C and H in methane (CH4).

b)

the H of one water molecule and the O of another water molecule.

c)

Na+and Cl- in salt.

d)

the two hydrogen atoms in a molecule of hydrogen gas (H2).

e)

Mg+and Cl- in MgCl2.

48.

Water is able to form hydrogen bonds because

a)

oxygen has a valence of 2.

b)

the water molecule is shaped like a tetrahedron.

c)

the bonds that hold together the atoms in a water molecule are polar covalent bonds.

d)

the oxygen atom in a water molecule has a weak positive charge.

e)

each of the hydrogen atoms in a water molecule is weakly negative in charge.

49.

What gives rise to the cohesiveness of water molecules?

a)

hydrophobic interactions

b)

nonpolar covalent bonds

c)

ionic bonds

d)

hydrogen bonds

e)

both A and C

50.

Which of the following effects is produced by the high surface tension of water?

a)

Lakes don't freeze solid in winter, despite low temperatures.

b)

A water strider can walk across the surface of a small pond.

c)

Organisms resist temperature changes, although they give off heat due to chemical reactions.

d)

Water can act as a solvent.

e)

The pH of water remains exactly neutral

51.

The bonds that are broken when water vaporizes are

a)

ionic bonds.

b)

hydrogen bonds between water molecules.

c)

covalent bonds between atoms within water molecules.

d)

polar covalent bonds.

e)

nonpolar covalent bonds

52.

Many mammals control their body temperature by sweating. Which property of water is most directly responsible for the ability of sweat to lower body temperature?

a)

water's change in density when it condenses

b)

water's ability to dissolve molecules in the air

c)

the release of heat by the formation of hydrogen bonds

d)

the absorption of heat by the breaking of hydrogen bonds

e)

water's high surface tension

53.

Buffers are substances that help resist shifts in pH by

a)

releasing H+ in acidic solutions

b)

donating H+ to a solution when they have been depleted.

c)

releasing OH- in basic solutions.

d)

accepting H+ when the are in excess.

e)

Both B and D are correct

54.

Which of the following statements is true about buffer solutions?

a)

They maintain a constant pH when bases are added to them but not when acids are added to them.

b)

They maintain a constant pH when acids are added to them but not when bases are added to them.

c)

They maintain a constant pH of exactly 7 in all living cells and biological fluids

d)

They maintain a relatively constant pH when either acids or bases are added to them.

e)

They are found only in living systems and biological fluids.

55.

Hydrophobic substances such as vegetable oil are

a)

nonpolar substances that repel water molecules.

b)

nonpolar substances that have an attraction for water molecules

c)

polar substances that repel water molecules

d)

ar substances that have an affinity for water.

e)

charged molecules that hydrogen-bond with water molecules.

56.

Why does ice float in liquid water?

a)

The liquid water molecules have more kinetic energy and thus support the ice.

b)

The ionic bonds between the molecules in ice prevent the ice from sinking.

c)

Ice always has air bubbles that keep it afloat.

d)

Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water

e)

The crystalline lattice of ice causes it to be denser than liquid water

57.

Temperature usually increases when water condenses. Which behavior of water is most directly responsible for this phenomenon?

a)

the change in density when it condenses to form a liquid or

b)

reactions with other atmospheric compounds

c)

the release of heat by the formation of hydrogen bonds

d)

the release of heat by the breaking of hydrogen bonds

e)

the high surface tension of water

58.

Which type of bond must be broken for water to vaporize?

a)

ionic bonds

b)

nonpolar covalent bonds

c)

polar covalent bonds

d)

hydrogen bonds

e)

covalent bonds

59.

Water's high specific heat is mainly a consequence of the

a)

small size of the water molecules.

b)

high specific heat of oxygen and hydrogen atoms.

c)

absorption and release of heat when hydrogen bonds break and form.

d)

fact that water is a poor heat conductor.

e)

inability of water to dissipate heat into dry air.

60.
Large bodies of water do not quickly fluctuate in temperature. Why?
a)
Water is a solvent.
b)
Water has a high heat capacity.
c)
Water acts as a buffer.
d)
Water is non-polar.
61.
What makes a molecule polar?
a)
Equal sharing of valence electrons
b)
Unequal sharing of valence electrons
c)
Stealing of electrons
d)
Temporary charges that come and go
62.

Water is an excellent solvent. Select the property that justifies this statement.

a)

as a polar molecule, it can surround and dissolve ionic and polar molecules

b)

it forms ionic bonds with ions, hydrogen bonds with polar molecules, and hydrophobic interactions with non polar molecules

c)

it forms hydrogen bonds with itself so cohesion is possible

d)

it is liquid and will adhere to many substances

63.

The partial negative charge at one end of a water molecule is attracted to a partial positive charge of another water molecule. What is this type of attraction called?

a)

a polar covalent bond

b)

an ionic bond

c)

a hydration shell

d)

a hydrogen bond

64.

What elements do carbohydrates contain?

a)

CHO

b)

CHON

c)

CHONP

d)

CHONPS

65.

An open system...

a)

Exchange matter only

b)

Exchange energy only

c)

Exchange matter and energy

66.

The smaller an animal is...

a)

The smaller the surface area to volume ratio

b)

The larger the surface area to volume ratio

67.

Smaller animals generally have a ______ metabolism

a)

Higher

b)

Lower

68.

Which type of chemical bond is formed when electrons are shared and is a stronger bond that is not easily broken?

a)

Ionic bond

b)

Covalent bond

c)

Hydrogen bond

d)

Van der Waals force

69.

Which type of water property explains water's ability to stick to other material.

a)

Cohesion

b)

Surface tension

c)

Adhesion

d)

High specific heat

70.

A material is hydrophobic, that means it...

a)

Doesn't mix with water or dissolve in water easily

b)

Mixes with water or dissolves in water easily

71.

An isotope has...

a)

The same numbers of neutrons and different numbers of protons

b)

The same numbers of electrons and different numbers of protons

c)

The same numbers of protons and different numbers of neutrons

d)

The same numbers of protons and different numbers of electrons

72.

Evaporative cooling

a)

Cools down an animal's body

b)

Cools down the environment

c)

Cools down both an animal's body and the environment

73.

Water is...

a)

Polar

b)

Nonpolar

74.
molecule that donates hydrogen ions and increases the concentration of hydrogen ions in a solution
a)
acid
b)
evaporation
c)
hydrophilic
d)
adhesion
75.
attraction between water molecules and other molecules
a)
adhesion
b)
buffer
c)
hydrogen bond
d)
specific heat capacity
76.
molecule that donates hydroxide ions or otherwise binds excess hydrogen ions and decreases the concentration of hydrogen ions in a solution
a)
base
b)
acid
c)
litmus paper (pH paper)
d)
specific heat capacity
77.
substance that resists a change in pH by absorbing or releasing hydrogen or hydroxide ions
a)
buffer
b)
sphere of hydration
c)
base
d)
surface tension
78.
occurs because water molecules are attracted to charges on the inner surfaces of narrow tubular structures such as glass tubes, drawing the water molecules to the sides of the tubes
a)
capillary action
b)
evaporation
c)
buffer
d)
cohesion
79.
intermolecular forces between water molecules caused by the polar nature of water; responsible for surface tension
a)
cohesion
b)
specific heat capacity
c)
heat of vaporization of water
d)
acid
80.
release of an ion from a molecule such that the original molecule now consists of an ion and the charged remains of the original, such as when water dissociates into H+ and OH-
a)
dissociation
b)
base
c)
electronegativity
d)
buffer
81.
ion necessary for nerve impulse conduction, muscle contractions and water balance
a)
electrolyte
b)
electronegativity
c)
sphere of hydration
d)
litmus paper (pH paper)
82.
ability of some elements to attract electrons (often of hydrogen atoms), acquiring partial negative charges in molecules and creating partial positive charges on the hydrogen atoms
a)
electronegativity
b)
specific heat capacity
c)
evaporation
d)
acid
83.
separation of individual molecules from the surface of a body of water, leaves of a plant, or the skin of an organism
a)
evaporation
b)
electronegativity
c)
buffer
d)
cohesion
84.
high amount of energy required for liquid water to turn into water vapor
a)
heat of vaporization of water
b)
hydrogen bond
c)
cohesion
d)
sphere of hydration
85.
weak bond between slightly positively charged hydrogen atoms and slightly negatively charged atoms in other molecules
a)
hydrogen bond
b)
sphere of hydration
c)
capillary action
d)
specific heat capacity
86.
describes ions or polar molecules that interact well with other polar molecules such as water
a)
hydrophilic
b)
adhesion
c)
evaporation
d)
hydrophobic
87.
describes uncharged non-polar molecules that do not interact well with polar molecules such as water
a)
hydrophobic
b)
litmus paper (pH paper)
c)
cohesion
d)
adhesion
88.
filter paper that has been treated with a natural water-soluble dye that changes its color as the pH of the environment changes so it can be used as a pH indicator
a)
litmus paper (pH paper)
b)
dissociation
c)
base
d)
acid
89.
scale ranging from zero to 14 that is inversely proportional to the concentration of hydrogen ions in a solution
a)
pH scale
b)
buffer
c)
evaporation
d)
heat of vaporization of water
90.
the amount of heat one gram of a substance must absorb or lose to change its temperature by one degree Celsius
a)
specific heat capacity
b)
sphere of hydration
c)
dissociation
d)
electronegativity
91.
when polar water molecules surround charged or polar molecules thus keeping them dissolved and in solution
a)
sphere of hydration
b)
dissociation
c)
heat of vaporization of water
d)
hydrogen bond
92.
tension at the surface of a body of liquid that prevents the molecules from separating; created by the attractive cohesive forces between the molecules of the liquid
a)
surface tension
b)
cohesion
c)
dissociation
d)
acid
93.
Which 4 elements make up most of all living matter?
a)
Carbon, Hydrogen, Nitrogen, Oxygen
b)
Carbon, Oxygen, Sodium, Potassium
c)
Carbon, Hydrogen, Calcium, Nitrogen
d)
Carbon, Oxygen, Nitrogen, Sulfur
94.
When atoms share electrons unequally...
a)
a nonpolar covalent bond is formed.
b)
an ionic bond is formed.
c)
a polar covalent bond is formed.
d)
a hydrogen bond is formed.
95.

A substance that cannot be decomposed into simpler substances by chemical means - made up of the same atoms

a)

atom

b)

element

c)

molecule

d)

organism

96.

A group of two or more atoms that are bonded together

a)

elements

b)

isotopes

c)

molecules

d)

essential elements of life

97.

An atom that has a different number of neutrons than the standard for that element.

a)

element

b)

isotope

c)

molecule

d)

organism

98.
What is the difference between carbon-12 and carbon-14? (Hint: 12 and 14 are mass #)
a)
The number of protons in the nucleus.
b)
The number of protons and neutrons in the nucleus.
c)
The number of neutrons in the nucleus.
d)
The number of electrons in the orbitals.
99.
Electrons have what charge?
a)
Negative
b)
Positive
c)
Neutral
 (No Charge)
100.
The nucleus of an atom is made up of...
a)
Protons and Neutrons
b)
Neutrons and Electrons
c)
Protons and Electrons
101.
The image shows the periodic grid for POTASSIUM. What is Potassium's atomic number?
a)
19
b)
39
c)
20
d)
Impossible to tell
102.
The image shows the periodic grid for POTASSIUM. How many ELECTRONS are found in a potassium atom?
a)
19
b)
39
c)
20
d)
Impossible to tell
103.
How many elements are represented in the compound?
Na2CO3
a)
1
b)
2
c)
3
d)
4
104.
Energy of motion is which type of energy?
a)
Potential
b)
Kinetic
c)
Sound
d)
Gravitational
105.
What kind of energy is represented in the picture?
a)
Thermal
b)
Chemical
c)
Sound
d)
Nuclear
106.
Stored energy is called ______ energy.
a)
Kinetic
b)
Potential
c)
Pacific
d)
Safe
107.
Atoms gain lose, gain, or ______electrons to get a stable outer energy level.
a)
share
b)
split
c)
create
d)
destroy
108.
An ionic compound is held together by the _______--the force of attraction between opposite charges of the atoms.
a)
Covalent Bond
b)
Ionic Bond
c)
Synthetic Bond
d)
Molecular Bond
109.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

110.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
111.

What is the greatest number of valence electrons an atom can have?

a)

2

b)

3

c)

8

d)

12

112.

TRUE OR FALSE:

Hydrogen bonds are very strong interactions between two atoms.

a)

True

b)

False

113.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
114.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
115.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
116.
What is the only substance with a neutral pH of 7?
a)
Milk
b)
Orange Juice
c)
Water
d)
Blood
117.
Complete the sentence.
A substance that is more basic has a _____ pH than a substance that is acidic.
a)
lower
b)
higher
c)
the same
d)
none of the above
118.

In a test of pH levels, a baking soda has a pH of 9 and bleach has a pH of 12. What is true about there relationship?

a)

Both of the solution are Bases

b)

Both of the solution are Acids

c)

The Baking soda is an acid and the Bleach is a base

d)

The baking soda is a base and the Bleach is an Acid.

119.
On the pH scale higher numbers indicate
a)
acids
b)
bases
120.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
121.
Bleach is a strong base, what is the pH level of bleach?
a)
13
b)
14
c)
1
d)
2
122.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

123.

Which of the following is the strongest acid?

a)

1

b)

5

c)

3

d)

8

124.

Which of the following is the strongest base?

a)

4

b)

14

c)

7

d)

15

125.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
126.
A neutralization reaction will always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
127.
A solution with a pH of 3.6 would be...
a)
Acid
b)
basic
c)
Neutral
d)
Acid and basic
128.
Is water a polar or non-polar molecule?
a)
polar
b)
non-polar
129.
What does the pH scale range from?
a)
0-10
b)
2-15
c)
1-5
d)
0-14
130.
What is cohesion?
a)
water molecules sticking to other water molecules
b)
water molecules sticking to different molecules
c)
when you dissolve a substance in a solution 
d)
when molecules become chemically combined
131.
what number is considered neutral on the pH scale?
a)
4
b)
12
c)
7
d)
10
132.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
133.
Why does ice float in water?
a)
Because of stronger hydrogen bonds at the surface
b)
The density of water as a solid is less than the density of water as a liquid
c)
Surface tension helps it float
d)
It is more dense
134.
What is an example of an organism that uses surface tension?
a)
a water llama
b)
a water strider
c)
a tadpole
d)
a snakehead
135.
What is the main property of water?
a)
Ice
b)
Adhesion
c)
Cohesion
d)
Polarity
136.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
137.
Bleach is a strong base, what is the pH level of bleach?
a)
13
b)
14
c)
1
d)
2
138.
What is a hydrogen bond?
a)
attraction between molecules of the same substance
b)
substance that is dissolved in a solution
c)
weak attraction between a hydrogen atom and another atom
d)
way plants transport water through their tissues
139.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 5
140.
Pollution causes the pH of rain water fall below 6. What is such type of rain called?
a)
Acid rain
b)
polluted rain
c)
low pH rain
d)
non-point source pollution
141.
A solution with a pH of 7.0 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
142.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons

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