Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

BIOLOGY 1002 Connect > Connect Homework > Flashcards

Connect Homework Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Biology flashcards Biology 101 flashcards
1
Q

Which subatomic particle is found in the space that surrounds the nucleus?

A

ELECTRON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

In a single element _____ type(s) of atoms can be found.

A

ONE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

A pure substance made up of only one atom is called a(n)?

A

ELEMENT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Which of the following best describes a contemporary model of electron movement within atoms?

A

Electrons move in orbitals, although their exact location cannot be precisely predicted in these orbitals.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Anything that contains mass and occupies space is called?

A

MATTER

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Within an atom’s structure, electrons can be found ______.

A

IN CLOUD LIKE ORBITALS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Which of the following is an element?

Gasoline, Coffee, Water, Carbon

A

CARBON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Orbitals are found in ______ or energy levels.

A

ELECTRON SHELLS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

True or false: An element is made up of two or more types of atoms?

A

FALSE ( An element is composed of only one kind of atom.)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Energy is defined as ______.

A

THE CAPACITY TO DO WORK

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Select all that apply

Which of the following are subatomic particles that are confined to a small volume within the nucleus of an atom?

  • Protons
  • Neutrons
  • Electrons
  • Prions
A

PROTONS AND NEUTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Chemical bonds can form among atoms due to the presence of unpaired _____ electrons

A

VALENCE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Here are three descriptions of the modern model of atomic structure. Which is the best?

  • A central nucleus surrounded by cloudlike orbitals containing electrons
  • A collection of positive and negative charges uniformly distributed throughout the atom
  • A central nucleus surrounded by electrons traveling in clearly defined orbits
A

A central nucleus surrounded by cloudlike orbitals containing electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What type of subatomic particle occurs in each different element in a unique number and is therefore used to identify specific elements?

A

PROTON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The region within an atom that surrounds the nucleus and in which there is a high probability of finding an electron is called an electron ____

A

ORBITAL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What does the atomic number of an atom represent?

A

THE NUMBER OF PROTONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Within atoms, electrons are organized by energy levels called?

A

ELECTRON SHELLS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

The capacity to do work is known as?

A

ENERGY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Select all that apply:

Select all of the following that are true about atoms that have partially filled energy shells.

A
  • Can form compounds

- Tend to share, lose, or gain electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Atoms of different chemical elements can be differentiated based on the number of ______ ?

A

PROTONS IN THE NUCLEUS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Electrons in an atom’s outermost energy shells are called ____ electrons?

A

VALENCE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

An atom’s atomic number is based on the number of ______
it contains. In an atom that is not in a chemical reaction, this number equals to the number of _____ ?
.

A

Blank 1: PROTONS

Blank 2: ELECTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Within an atom, particles with nearly equal mass are ____ and neutrons, while _____ have a much smaller mass.

A

Blank 1: PROTONS

Blank 2: ELECTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Orbitals are found in ______ or energy levels.

A

ELECTRON SHELLS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

An element’s atomic ______ is based on the protons and neutrons it contains, while an element’s atomic ______ is based only on the number of protons.

A

Blank 1: MASS

Blank 2: NUMBER

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

The most common type of carbon atom has 6 protons, 6 electrons, and 6 neutrons. What is its atomic mass?

A

12 AMU or 12 DALTONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Valence electrons are found in ______.

A

THE OUTERMOST ENERGY SHELL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Atomic mass is measured in what units?

A

AMU (atomic mass units)

DA (Daltons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Which two particles are the primary determinants of an element’s atomic mass?

A

PROTONS AND NEUTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Phosphorus exists in several isotopes, including 31P and 32P. These are expected to have different ______.

A

NUMBER OF NEUTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

The atomic number of an element is equal to the number of ____
it contains. Its atomic mass includes the number of protons and the number of ____

A

Blank 1: Protons

Blank 2: Neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What four elements are the most common in living organisms?

A

OXYGEN, CARBON, HYDROGEN, NITROGEN

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Oxygen has eight protons, 8 electrons, and 8 neutrons. What is its atomic mass?

A

16

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Water, with the chemical formula H2O, contains ____ hydrogen atom(s) and _____ oxygen atom(s).

A

Blank 1: 2

Blank 2: 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Atoms share a pair of electrons when they form a(n) ____ bond.

A

COVALLENT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

One ______ equals 1/12 the mass of a carbon atom.

A

DALTON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

In which of the following scenarios are atoms the most stable?

A

When their outer shells are filled with electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Isotopes of an element differ from one another in the number of ____
they contain.

A

NEUTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Why are atoms likely to share electrons?

A

Because they have unfilled outer valence shells.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

By mass, the most abundant element in living organisms is ______.

A

OXYGEN

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What is a likely predictor of how many covalent bonds an atom can form?

A

The electron configuration in the outermost shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

The chemical formula of glucose is C6H12O6. How many oxygen atoms are in one molecule of glucose?

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

According to the octet rule, many atoms are most stable when they have ______ electrons in their outermost shell?

A

8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

A covalent bond is one in which a pair of electrons ______.

A

is shared between 2 atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Electronegativity is the ability of an atom to ______.

A

attract electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Atoms are most stable when their outer shells are filled with?

A

electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What is true of a polar covalent bond?

A
  • The two atoms in the bond share the electrons unequally

- The atoms in the bond differ in electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

Atoms tend to be most stable when their outer shells are _____ ; this can be accomplished by gaining, losing, or sharing _____.

A

Blank 1: Filled

Blank 2: Electrons or Valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

Nitrogen has five electrons in its outer shell, so it can bond with up to ______ other atoms to complete its outer shell?

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

A covalent bond in which the atoms share electrons unequally is a(n) _____
covalent bond.

A

Polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

Atoms are chemically the most stable when which of the following occurs?

A

Their outer shell is full.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

The hydrogen bonds connecting water molecules form between a(n) ______ atom on one molecule and a(n) ______ atom on another molecule.

A

Blank 1: oxygen

Blank 2: hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

The measure of an atom’s ability to attract electrons when in a bond with another atom is called its ______?

A

Electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

What best describes how a hydrogen bond forms?

A

A partially positive hydrogen atom and a partially negative atom in another molecule are attracted by electrostatic interactions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

A(n) ______ bond is formed when two atoms of different electronegativities share electrons.

A

Polar covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

Why are atoms likely to share electrons?

A

Because they have unfilled outer valence shells.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

An atom that has gained or lost electrons, and thus has a net electric charge, is called a(n)

A

Ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

In a polar covalent bond, the shared electrons are closer to the nucleus of the atom with ______.

A

Greater electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

If an atom gains or loses a(n) _____ it acquires a net electrical charge and becomes an ion.

A

Electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

When two water molecules are near each other, a hydrogen bond will form between the more positive _____ and the more negative _____
atoms of neighboring water molecules.

A

Blank 1: Hydrogen

Blank 2: Oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

Anions are types of ions that have a net ____ charge.

A

Negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

A hydrogen bond forms when a hydrogen atom with a partial ____ charge becomes electrically attracted to an electronegative atom with a partial ____ charge.

A

Blank 1: Positive

Blank 2: Negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

Which of the following statements are true of a polar covalent bond?

A
  • The two atoms in the bond share the electrons unequally.

- The atoms in the bond differ in electronegativity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

An atom with a net electric charge is called a(n) ______.

A

Ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
64
Q

Molecules with covalent bonds ______.

A

Are flexible within certain limits

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
65
Q

A Na+ ion forms when a sodium atom ______.

A

Loses an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
66
Q

An ion that carries a net negative charge is a(n) ______.

A

Anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
67
Q

A(n) ____ containing an atom with a single, unpaired electron in its outer shell is known as a free radical.

A

Molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
68
Q

An atom or ion is most stable when its outermost shell is occupied by its full complement of ____.

A

8 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
69
Q

Which of the following are common features of chemical reactions?

A
  • Chemical reactions require a source of energy.
  • Many chemical reactions in living organisms take place in a watery environment.
  • Chemical reactions proceed toward equilibrium.
  • Many chemical reactions that occur in cells require catalysts.
70
Q

True or false: Molecules that contain covalent bonds are rigid, inflexible structures.

A

False

71
Q

Which of the following properties are shared by many chemical reactions that occur in cells?

A
  • They tend to proceed toward equilibrium.
  • They require energy.
  • They often require a catalyst.
72
Q

A free radical is a molecule containing an atom with a single unpaired electron in its ______.

A

Outer shell

73
Q

In which of these conditions would an atom or ion be most stable?

A

When its outermost shell is occupied by its full complement of electrons

74
Q

Consider the reaction: CH4 + 2 O2 ⇌ CO2 + 2 H2O. Oxygen serves as a(n) ______.

A

Reactant

75
Q

What occurs during all chemical reactions?

A

Chemical bonds are broken or formed.

76
Q

In a chemical reaction, if there is no longer a change in the concentration of reactants and products, then ______.

A

Equilibrium has been reached

77
Q

Which component of humans has the greatest percent of water?

A

Lungs

78
Q

Chemical reactions require a source of energy and also may require a substance called a(n) ____ that speeds up the reaction rate. Most chemical reactions proceed toward a state called ____ in which the rate of product formation equals the rate of reactant formation.

A

Blank 1: Catalyst

Blank: Equilibrium

79
Q

Substances dissolved in liquid are called ______.

A

Solutes

80
Q

A solution is composed of ______ dissolved in a ______.

A

solutes; solvent

81
Q

In the conversion of methane and oxygen to carbon dioxide and water, carbon dioxide is a(n) ______.

A

Product

82
Q

A solution in which water is the solvent is called a(n)

A

Aqueous

83
Q

When the rate of the forward reaction is equal to the rate of the reverse reaction, chemical ____ has been reached.

A

Equilibrium

84
Q

In a micelle, which portion of the amphipathic molecules are oriented toward the surface of the sphere?

A

The polar region

85
Q

In humans, water comprises approximately ______ of body weight.

A

60-70%

86
Q

The concentration of a liquid is defined as the amount of ______ dissolved in a unit volume of solution.

A

Solute

87
Q

A liquid that can dissolve substances is known as a(n) ____

A

Solvent

88
Q

Solutes dissolved in a solvent form a ______.

A

Solution

89
Q

The molecular mass of a molecule is equal to the ______ in the molecule.

A

Sum of the atomic masses of all atoms

90
Q

An aqueous solution is one in which the solvent is ______.

A

Water

91
Q

Put the physical states of water in order based on the intermolecular distances between water molecules. The TOP position should be the state in which the molecules are the farthest apart.

A

1) The Gaseous state
2) The Solid state
3) The Liquid state

92
Q

What part of an amphipathic molecule would be oriented toward the center of a micelle?

A

The nonpolar region

93
Q

The amount of solute (in grams) dissolved in a given volume of solution is the solution’s ______.

A

concentration

94
Q

Why does ice float in liquid water?

A

Ice is less dense than liquid water.

95
Q

When water is heated, the rate at which ____ bonds break increases, and water molecules are converted to the ____.

A

Blank 1: Hydrogen

Blank 2: Gaseous

96
Q

The sum of the atomic masses of all atoms in a molecule is equal to the molecule’s ____ mass.

A

Molecular

97
Q

Which state of water is the most dense?

A

Liquid

98
Q

Compared with liquid water, ice has ______.

A
  • More hydrogen bonds between individual water molecules

- A more orderly arrangement of water molecules

99
Q

Ice floats in liquid water because ice has a lower ______ than liquid water.

A

Density

100
Q

Which of the following changes in the physical state of water require the input of energy?

A
  • Changing from liquid to gas

- Changing from solid to liquid

101
Q

What happens when water freezes?

A
  • Water molecules are packed into a less dense formation.
  • The rate of hydrogen bond breakage slows.
  • The H2O molecules in ice are in a much more orderly arrangement than in the liquid state.
102
Q

Rank each state of water in order of increasing density, starting with the least dense state at the top of the list.

A

1) Water vapor
2) Ice
3) Liquid water

103
Q

What is the heat of fusion of a substance?

A

The amount of heat energy released when 1 mole of the substance is converted from liquid to solid

104
Q

______ is the amount of energy required to raise the temperature of 1 gram of a substance by 1o C

A

Specific heat

105
Q

Properties of a solution that depend strictly on the total number of dissolved solutes, and not the specific type of solute, are called ____ properties.

A

Colligative

106
Q

To freeze water, energy is ______.

A

Released

107
Q

Water is used to break apart another molecule in a(n) ____ reaction.

A

Hydrolysis

108
Q

High specific heat, surface tension, and cohesion are several properties of water involving ____ bonds.

A

Hydrogen

109
Q

What is heat of vaporization?

A

The heat energy required to convert 1 mole of a substance from liquid to gas

110
Q

What is heat of fusion?

A

The heat energy that must be withdrawn or released from a substance to convert it from liquid to solid

111
Q

What is specific heat?

A

The heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius

112
Q

What is heat Capacity?

A

The heat energy required to raise the temperature of an entire object

113
Q

Pure water can ionize into which of the following?

A

Positively charged protons (H+) and negatively charged hydroxide (OH-) ion

114
Q

pH is defined as the ____ ____ to the base 10 of the ____ ion concentration.

A

Blank 1: negative
Blank 2: logarithm
Blank 3: Hydrogen

115
Q

Colligative properties depend on the ______ dissolved in a solution.

A

Number of particles

116
Q

What happens to the pH of a solution when H+ ions are added to it?

A

The pH decreases

117
Q

Hydrolysis reactions ______.

A

Break apart molecules via water

118
Q

A solution at pH 5 is said to be ______ because it contains more ______.

A

Blank 1: Acidic

Blank 2: (Hydrogen) H+ ions than (Hydroxide) OH- ions

119
Q

Polar covalent O-H bonds in water molecules enable hydrogen bonds to form between water molecules. Which of the following properties of water result from hydrogen bond formation?

A
  • Cohesion
  • High heat of vaporization
  • Surface tension
  • High specific heat
  • Adhesion
120
Q

Which ions are produced when water ionizes?

A
  • H+ ( Hydrogen)

- OH– (Hydroxide)

121
Q

What type of compound minimizes pH fluctuations in the fluids of living organisms?

A

Buffer

122
Q

The ______ of a solution is the negative base 10 logarithm of the H+ concentration of the solution.

A

pH

123
Q

If you add H+ ions to a solution, it becomes more ______.

A

Acidic

124
Q

Which of the following solutions contains the highest concentration of protons?

A

A solution with pH 2.0

125
Q

A ____________ of a substance contains the same number of particles as there is in 12g of carbon.

A

Mole

126
Q

One ____________ is approximately the mass of one proton or a hydrogen atom.

A

Dalton

127
Q

The ____________ of an atom is a relative measure of its mass compared to other atoms.

A

Atomic Mass

128
Q

____________ of carbon = 1 mole.

A

12g

129
Q

____________ of hydrogen = 1 mole

A

1g

130
Q

____________ of lithium = 1 mole.

A

7g

131
Q

Hydrogen has a total of ____________ electron(s), ____________ are in the valence shell, and ____________ lie in the p orbitals.

A

1, 1, 0

132
Q

Carbon has a total of ____________ electron(s), ____________ are in the valence shell, and ____________ are in the 1s orbital.

A

6,4,2

133
Q

Nitrogen has a total of ____ electron(s), ____ are in the valence shell, and ____ lie in the p orbitals.

A

7,5,3

134
Q

Oxygen has a total of ____________ electrons, ____________ are in the valence shell, and ____________ are in the p orbitals.

A

8,6,3

135
Q

These 2 have the same number of electrons in their outermost shells.

A

Nitrogen & Phosphorus

136
Q

These 2 have two electron shells.

A

Carbon & Nitrogen

137
Q

Their outermost electron shell is full.

A

Helium & Argon

138
Q

They have one electron shell.

A

Hydrogen & Helium

139
Q

hey have three electron shells.

A

Sodium & Chlorine

140
Q

Which two elements show similarities in the pattern of chemical bonding?

A

Lithium and Sodium

141
Q

A polar covalent bond is created when

A

Bonded atoms have unequal pull on the shared electron, so that the electron spends more time around one atom than the other.

142
Q

The unequal sharing of electrons between the oxygen and hydrogen atoms within a water molecule makes water a ____________ molecule.

A

Polar

143
Q

As a result of the electron configuration of a water molecule, water is a great ____________ because water can break up and surround a ____________ , as long as it is not ____________ , dissolving it into solution.

A

Solvent, Solute, nonpolar

144
Q

The reason water behaves in this manner is because the ____________ charge on the hydrogen end of the water molecule is attracted to the negative charge of a polar molecule, while the ____________ charge of the oxygen end of the water molecule is attracted to the positive side of a polar molecule.

A

Positive, Negative

145
Q

True or False: The bonds between water molecules are stable.

A

False

146
Q

True or False: As temperature drops the bonds between water molecules are less likely to break.

A

True

147
Q

True or False: Ice is denser than liquid water at all temperatures

A

False

148
Q

True or False: The polar covalent bonds between hydrogen and oxygen atoms within a water molecule create slight positively and negatively charged ends to the molecule

A

True

149
Q

True or False: The fluid nature of water is due to hydrogen bonds continually breaking and reforming.

A

True

150
Q

True or False: A hydrogen atom of one water molecule binds via a hydrogen bond to a hydrogen atom of another water molecule.

A

False

151
Q

True or False: Bonds between water molecules are stronger than the bonds between the atoms within a water molecule.

A

False

152
Q

Decide which example best describes each property of water.

1. Water is less dense at 0°C compared to 4°C.

A

Ice floats

153
Q

Decide which example best describes each property of water.

2. Water provides structural support due to its inability to be compressed.

A

Turgid pressure in plants

154
Q

Decide which example best describes each property of water.

3. The charged ends of a water molecule allow it to surround a solute in solution.

A

Solvent

155
Q

Decide which example best describes each property of water.
4.The temperature of water rises slowly due to its high specific heat; requiring a lot of energy to convert liquid water to water vapor.

A

Evaporative cooling

156
Q

Decide which example best describes each property of water.
5. While hydrogen bonds are constantly breaking and reforming, a large percentage of the hydrogen bonds between water molecules exist at all times.

A

Cohesive force

157
Q

Decide which example best describes each property of water.

6. Due to hydrogen bonding, water tends to adhere to surfaces, such as the lining of the digestive tract.

A

Lubricant

158
Q

Decide which example best describes each property of water.

7. The addition of water can break apart molecules into two smaller molecules.

A

Hydrolysis

159
Q

Decide which example best describes each property of water.

8. Water is formed when two molecules come together to form a large molecule.

A

Dehydration reaction

160
Q

The ____________ of water molecules, resulting from the ____________ bonds between water molecules, causes a movement of the water through the plant’s vessels, as it moves up from the roots.

A

Cohesion; Hydrogen

161
Q

As water ____________ from the pores of the leaves, more water is pulled up from below resulting in a constant supply of water moving up through the vessels of a plant.

A

Evaporates

162
Q

Trees take up water from their roots. Water must travel against ____ up to all of the branches and leaves.

A

Gravity

163
Q

6 CO2 + 6 H2O + Light → C6H12O6 + O2 is an example of a chemical reaction. What is occurring during this reaction?

A

Substances are changed into other substances by the making or breaking of chemical bonds.

164
Q

Adding NH3 (ammonia) to water makes NH4+. What will be the general pH of this new solution, and what will happen to the ion concentrations?

A

Alkaline; decreased H+ ions and increased OH- .

165
Q

Stable blood serum has a pH of around 7.4. The release of bicarbonates as a buffer to maintain this pH in a body with high hydrogen levels would cause the pH to move

A

From acidic to slightly alkaline.

166
Q

The property of water that allows the basilisk lizard to run across its surface is

A

The high surface tension caused by the polar qualities of water.

167
Q

The best summary of the properties of water is

A

less dense at 0oC than at room temperature, ideal solvent for biological molecules, absorbs considerable heat energy without raising temperature, and high percentage of hydrogen bonds.

168
Q

When H2O is added to a compound in a chemical equation, a new compound can be formed via what type of reaction?

A

Hydrolysis

169
Q

When two atoms are bonded together via electrons, and one of those atoms has a greater pull upon the electrons shared, the bond formed would be

A

A polar covalent bond.

170
Q

Carbon 12, 13, and 14 are isotopes of the same element. They share the same place on the periodic table but possess varying numbers of neutrons. If carbon 12 has 6 protons, how many neutrons will carbon 14 have?

A

8

171
Q

Water (H2O) is critical to sustain life. One of its major roles is creating and breaking bonds in chemical reactions. Other significant roles of water include

A
  • acting as a solvent in the transport of dissolved substances around the body.
  • the protection and support of organs.
  • maintaining body temperature homeostasis.
172
Q

Electrons that orbit the nucleus of an atom

A
  • Require input of discrete amounts of energy to move between shells.
  • Have lower potential energy as they move closer to the nucleus.
173
Q

What element is found in all organic molecules?

A

Carbon

BIOLOGY 1002 Connect (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions