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Biology Honors (9) > Chapter 2: The Chemistry of Life > Flashcards

Chapter 2: The Chemistry of Life Flashcards

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1
Q

What three subatomic particles make up atoms?

A

Protons, neutrons, electrons

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2
Q

What do protons give an atom?

A

Its identity

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3
Q

What do electrons give to atoms?

A

Its ‘personality’

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4
Q

What is a cell?

A

The basic building block of living organisms

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5
Q

What is an atom?

A

The basic building block of matter

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6
Q

Which particle(s) are in the nucleus?

A

Neutrons, protons

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7
Q

Which particle(s) are not in the nucleus?

A

Electrons

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8
Q

What is an element?

A

substance that cannot be decomposed into simpler substances by chemical means & has atoms made with identical number of protons

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9
Q

Elements are made up of atoms all with the identical number of _____.

A

Protons

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10
Q

Atomic number

A

of protons of an atom

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11
Q

Atomic Mass

A

Average mass of all atoms of an element

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12
Q

Mass number

A

of protons + neutrons

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13
Q

Charge

A

Indicates a gain or loss of electrons (ions)

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14
Q

How big is 1 proton?

A

1 amu

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15
Q

How big is 1 neutron?

A

1 amu

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16
Q

How big is 1 electron?

A

nothing (1/1840 the size of a proton or neutron)

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17
Q

Isotopes are atoms of the ___ element with a different number of _____.

A

Same, Neutrons

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18
Q

Radioactive decay

A

breakdown of the nucleus of an atom

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19
Q

What is a radioactive isotope?

A

Isotopes where the nucleus is UNSTABLE and breaks down at a constant rate over time

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20
Q

Half-life

A

Constant rate where isotope of the nucleus breaks down. Can be used to figure out ages of elements using graphs.

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21
Q

3 ways to use radioactive isotopes

A
  • cancer treatment
  • tracers (radioactive elements)
  • dating rocks/organic remains
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22
Q

What is a substance?

A

That which has mass and occupies space; matter.

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23
Q

A substance is _____ meaning it is a material with a particular kind.

A

PURE

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24
Q

What is a chemical compound?

A

A substance; formed by the chemical combination of two or more elements

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25
Q

What is a molecule?

A

A compound that is bound together by covalent bonds.

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26
Q

What is an IONIC compound?

A

A compound bound that is held together by ionic bonds.

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27
Q

What does the octet rule say?

A

Atoms tend to gain, lose or share electrons so that they have 8 electrons in their outer electron shell.

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28
Q

What are valence electrons?

A

The outermost shell of electrons

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29
Q

True or False; Sodium is a pure substance.

A

True

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30
Q

What type of element is sodium? What is its atomic number?

A

soft metal (alkali metal); atomic number is 11

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31
Q

What type of element is chlorine, and what is its atomic number?

A

pure substance; poisonous gas. its atomic number is 17.

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32
Q

Sodium + Chloride = _____

A

Salt (NaCl), an ionic bond

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33
Q

What are ionic bonds?

A

A bond between atoms when electrons are transferred from one atom to another

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34
Q

What are ions?

A

positive or negatively charged atoms

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35
Q

Describe a cation.

A

loses electrons, creates positive ion

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36
Q

Describe an anion.

A

gains electrons, creates negative ion

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37
Q

What are covalent bonds?

A

Bonds with electrons that are shared by atoms

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38
Q

Define single, double, and triple covalent bonds.

A

Single: Share 2 electrons
Double: 4 electrons
Triple: 6 electrons

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39
Q

What is electronegativity?

A

The want for electrons.

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40
Q

Why is a water molecule polar?

A

There is an uneven distribution of electrons between oxygen and hydrogen atoms.

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41
Q

Hydrogen bonds are a type of ____ force.

A

Van Der Waals.

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42
Q

Which is stronger? Hydrogen Bonds vs covalent/ionic bonds

A

covalent and ionic bonds

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43
Q

_____ creates magnet effect.

A

Polarity of water

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44
Q

What is the difference between cohesion and adhesion?

A
  • Cohesion is the attraction between molecules of the SAME substance.
  • Adhesion is the attraction between molecules of different substances.
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45
Q

Combination of cohesion and adhesion

A

Capillary action

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46
Q

Capillary action is: ____ of ____ to itself and _______ b/w water and ______ causes water to rise in a narrow tube against gravity.

A

Cohesion, water, adhesion, glass

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47
Q

Water drawn out form the roots of a plant to its stems and leaves is an example of? (cohesion, adhesion, capillary action)

A

CAPILLARY ACTION

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48
Q

Water has a (low/high) specific heat capacity. What does this mean?

A

high. it takes more energy to increase the temperature of water compared to other substances.

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49
Q

Specific heat

A

energy needed to raise temperature of 1 gram of a substance by 1 degree Celcius.

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50
Q

Why does water expand as it freezes?

A

Water is a polar molecule.

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51
Q

Mixture

A

Material composed of 2 or more elements which can be physically separated

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52
Q

Solution

A

Mixture where all components are evenly distributed

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53
Q

Suspension

A

Mixture that contains non-dissolved materials (not evenly distributed)

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54
Q

Solute vs solvent

A
  • Solute is the substance dissolved
  • Solvent is the substance in which the solute dissolves in
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55
Q

What important fluid contains both solutions and suspensions?

A

Blood

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56
Q

Chemical equation for forming water

A

2 H2 + 1 O2 = 2 H2O
water = hydroxide ion + hydrogen ion

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57
Q

what does pH stand for?

A

Power of Hydrogen

58
Q

What does the pH scale measure?

A
  • the concentration of hydrogen ions (H+) in a solution. 0-14
59
Q

What is the difference between Acids VS Bases?

A
  • Acids have HIGHER concentrations of H+ ions than pure water. pH < 7
  • Bases have LOWER concentrations of H+ ions than pure water. pH > 7
60
Q

Buffer

A

weak acid or base that helps react with strong acids to prevent strong sudden changes in pH. (ex: helping with heartburn)

61
Q

as pH increases by 1, the concentration of H+ ions ______ by a factor of ____.

A
  • decreases
  • 10x
62
Q

What are the 4 main types of macromolecules?

A
  • Carbohydrates
  • Lipids
  • Proteins
  • Nucleic Acid
63
Q

Organic chemistry is the study of ____ compounds.

A

Carbon

64
Q

List 4 ways why it is so important to study the carbon atoms.

A
  • It contains four valence electrons
  • Four covalent bonds
  • Can bonds with many elements Carbon can bond to sulfur, hydrogen, oxygen, phosphorous, sulfur, and nitrogen.
  • Carbon also bonds with other carbon atoms.
65
Q

Macromolecules

A

“giant molecules” formed from smaller molecules

66
Q

Monomers

A

Smaller units which are joined together to form polymers

67
Q

Polymerization

A

Monomers joining together to form polymers

68
Q

Carbohydrate

A
  • Usually in a 1:2:1 ring shape
  • Main source of energy
69
Q

Define monosaccharides, disaccharides, and polysaccharides.

A

Monomer, dimer, polymer.

70
Q

Give 4 examples of monosaccharides.

A

Fructose, glactose, ribose, deoxyribose

71
Q

Give 3 examples of disaccharides.

A

Sucrose, Lactose, Maltose

72
Q

What suffix means related to sugar?

A

-ose

73
Q

Name 4 types of polysaccharides (and expand their definitions)

A
  • Cellulose (plant cell walls)
  • Plant Starch (energy source of flour, bread, pasta)
  • Chitin (exoskeleton of anthropods)
  • Glycogen (animal starch, energy storage)
74
Q

What is the dehydration synthesis?

A

Removal of water to join MONOMERS together

75
Q

What is hydrolysis?

A

the “opposite” of dehydration synthesis. ADDITION of water to break POLYMERS apart.

76
Q

What’s the chemical process of the dehydration synthesis?

A

amino acid + amino acid -> peptide + water

77
Q

What are lipids (fats) made of?

A

Glycerol heads (hydrophillic), Fatty acid tails (hydrophobic)

78
Q

What are two functions of lipids?

A
  • to store energy
  • cell membranes
  • protection brain/nervous system
  • hormones
79
Q

What are two key types of lipids?

A

triglycerides, phospholipids

80
Q

What is the chemical process of ester bonds?

A

glycerol + fatty acids -> triglyceride

81
Q

What involves the process of glycosidic bonds?

A

when SUGARS are joined together

82
Q

What involves the process of peptide bonds?

A

when AMINO ACIDS are joined together

83
Q

Saturated fat

A

Full of hydrogen, no double bonds

84
Q

Unsaturated fat

A

one double bond

85
Q

Polyunsaturated fat

A

more than one double bond

86
Q

In nucleic acids, what are the monomers?

A

nucleotides

87
Q

In nucleic acids, what are the polymers?

A

nucleic acids (DNA/RNA)

88
Q

What is the function of nucleic acids?

A

they store and transmit hereditary/genetic information.

89
Q

What does each nucleotide contain?

A
  • 5-carbon sugar as ribose or deoxyribose
  • phosphate group
  • nitrogenous base
90
Q

What sugar does DNA use?

A

deoxyribose

91
Q

What sugar does RNA use?

A

Ribose

92
Q

What does ATP stand for?

A

Adenosine triphosphate (energy carrier)

93
Q

What are the monomers of protein?

A

Amino acids. There are 20 amino acids, and 9 essential amino acids.

94
Q

What are the polymers of protein?

A

protein (polypeptides)

95
Q

What is the chemical formula for peptide formulas?

A

amino acid 1 + amino acid 2 -> water + dipeptide

96
Q

What are the levels of organization of a protein?

A
  • Primary structure - sequence of its amino acids
  • Secondary structure - folding or coiling of the polypeptide chain
  • tertiary structure - protein starts to wrap and fold around itself, complete 3d arrangement
  • quaternary structure - protein starts to fold and wrap around other proteins
97
Q

What is the dehydration synthesis process of a lipid?

A

glycerol + fatty acids -> triglyceride + 3 water molecules

98
Q

ATP vs ADP

A

ATP is a “fully charged” battery compared to ADP, which is a partially charged battery.

99
Q

Which molecule contains sugar, a phosphate group, and a nitrogenous base?
(Proteins, lipids, carbohydrates, nucleic acids)

A

nucleic acids

100
Q

What is likely to be a good energy source for an organism? Carbs/lipids?

A

carbohydrates; easier to metabolize, more healthier than fat and oil.

101
Q

what suffix means to split or separate?

A

-lysis

102
Q

Variable

A

a condition that may cause a change in the system being studied.

103
Q

Controlled experiment

A

only one experiment is changed to ensure that the effect of only variable can be measured

104
Q

Independent variable

A

changed by the experimenter during the experiment

105
Q

Dependent variable

A

What changes as a result of the change in the independent variable

106
Q

Controlled variables

A

kept constant in each trial as it does not affect the outcome of the experiment

107
Q

Control group

A

set of organisms or samples that do not receive the treatment (independent variable) that is being tested

108
Q

Isomer

A

compounds with the same formula but a different arrangement of atoms in the molecule and different properties

109
Q

Is a water molecule neutral or charged? Why?

A

A water molecule is neutral, because it has 10 protons and 10 electrons.

110
Q

Give an example of cohesion.

A

water sticking to itself, surface tension

111
Q

Give an example of adhesion.

A

meniscus of graduated cylinder

112
Q

Give examples for mixtures.

A

lemonade, salt water, salad dressing

113
Q

Give an example of a solute.

A

table salt in saltwater

114
Q

Give an example of a solvent.

A

water in a saltwater solution

115
Q

Suspension example

A

mud in pond water, paint

116
Q

Solution Example

A

salt being dissolved in water

117
Q

Identify some real life acids.

A

lemon, apple, banana, vingear, tomato, milk, hydrochloric acid

118
Q

Identify some real life bases.

A

baking soda, blood, soap, ammonia, drain cleaner

119
Q

Saturated solution

A

when a given amount of water has dissolved all of the solute it can

120
Q

CHO

A

Carbohydrate, lipids

121
Q

CHON

A

proteins

122
Q

CHONP

A

Nucleic Acid

123
Q

Exergonic reaction

A

releases energy, usually occurs spontaneously (ex: cellular respiration)

124
Q

Endergonic reaction

A

absorbs energy, doesn’t occur spontaneously (ex: photosynthesis)

125
Q

Activation energy

A

energy required to get a chemical reaction started

126
Q

What are catalysts?

A

A substance that speeds up the rate of a chemical reaction

127
Q

What are enzymes?

A

Enzymes are proteins that act as a biological catalyst

128
Q

Substrate

A

The reactant that an enzyme acts on

129
Q

Enzyme-substrate complex

A

The enzyme binds to its subtrate, forming an enzyme-substrate complex

130
Q

active site

A

the region on the enzyme where the substrate binds

131
Q

Induced fit

A

Brings chemical groups of the active site into positions that enhance their ability to catalyze the reaction

132
Q

The active site can lower an E_a barrier by

A
  • orienting substrates
  • straining substrate bonds
  • providing a favorable microenvironment
  • covalently bonding to the substrate
133
Q

What can be used to regulate enzyme activity?

A
  • temperature
  • pH
  • activators
  • inhibitors
134
Q

Denature

A

Enzyme loses its organized shape and can no longer function, because of drastic changes

135
Q

Competitive inhibition

A

blocking molecule

136
Q

Noncompetitive inhibition

A

Allosteric regulation; “on” and “off” keys (binding proteins)

137
Q

Why does ice float on water?

A

Ice expands while it freezes, and this occurs because of the polarity of water, which occurs from the bent structure of water. This causes the hydrogen bonds to form and open network and make ice less denser than water.

138
Q

What are the monomers of carbohydrates?

A

Monosaccharides

139
Q

What are the monomers of lipids? What are the polymers?

A

fatty acids and glycerol heads. Triglycerides and phospholipids.

140
Q

What are the functions of proteins?

A
  • form cellular structures
  • control rate of reactions
  • regulate cell processes
141
Q

What are the essential elements of PROTEINS (amino acids)?

A
  • Carboxylic acid group
  • Amine group
  • Variable R side chain

Biology Honors (9) (7 decks)

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