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Bio HO9 > Chapter 2.1, 2.2 and 2.3 > Flashcards

Chapter 2.1, 2.2 and 2.3 Flashcards

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1
Q

Organic Chemistry

A

the study of compounds that contain bonds between carbon atoms

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2
Q

Inorganic Chemistry

A

the study of all other compounds that do not include carbon

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3
Q

Why is carbon so important?

A

1) Carbon has four valence electrons -> it can form strong covalent bonds with many other elements.2) Carbon can bond with carbon3) Carbon is extremely versatile and can bond in many ways and in many shapes4) Carbon makes up all life

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4
Q

Macromolecule

A

(very big polymer) Giant molecules, which are made up of thousands of smaller molecules. Make up most organic compounds on living cells. They are sorted into groups by chemical compounds.

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5
Q

How are macromolecules formed?

A

through polymerization

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6
Q

What is polymerization?

A

the process by which smaller compounds are joined toegther to make larger ones

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7
Q

Smaller compounds that join together to form larger ones are called….

A

monomers

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8
Q

What do monomers form?

A

polymers

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9
Q

The monomers in a polymer must always be identical.(True or False)

A

False; they can be different or identical

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10
Q

How many major groups are the macromolecules sorted into?

A

4

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11
Q

What are the major groups that macromolecules are sorted into?

A

Carbohydrates, lipids, nucleic acids, and proteins

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12
Q

What are carbohydrates made of?

A

carbon, hydrogen, and oxygen atoms usually in a ratio of 1:2:1(Ex: [CH2O]n) {little n is a variable that represents a number between 3-8, which you can plug into the 1:2:1 ratio}

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13
Q

What is the purpose of carbohydrates?

A

Carbohydrates are the main source of energy of living things; some organisms (such as plants) use them for structural purposes; some use for storage of energy

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14
Q

What are the two categories of carbohydrates?

A

Simple sugars and complex carbohydrates

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15
Q

How are carbohydrates formed?

A

Through dehydration synthesis

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16
Q

What are simple sugars?

A

monosaccharides such as glucose, galactose, fructose, etc.

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17
Q

Monosaccharides

A

single sugar molecules(Ex: Glucose)

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18
Q

Disaccharides

A

compound made by 2 simple sugars(Ex: sucrose)

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19
Q

What are complex carbohydrates?

A

(aka polysaccharides) large macromolecules formed from Monosaccharides

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20
Q

Examples of complex carbohydrates

A

starch, glycogen, cellulose

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21
Q

Starch

A

formed when glucose molecules join together in long chains

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22
Q

Isomer

A

Elements with the same number/type of atoms, but different chemical formulas -> therefore they have different shapes and functions

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23
Q

Glycogen

A

(aka animal starch) long chains of glucose where animals store excess sugar.

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24
Q

Cellulose

A

structural polysaccharides that give plants their strength and rigidity

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25
Q

What are lipids

A

a large and varied group of biological molecules that is usually not soluble in water. l only macromolecule not made of monomers l fat molecule l can be used to store energy and are an important part of membranes, waterproof coverings, fats, oils,and waxes

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26
Q

How are lipids formed?

A

Through dehydration synthesis

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27
Q

What are lipids made of?

A

Made of glycerol and fatty acids (carbon and hydrogen atoms)

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28
Q

Saturated

A

If there is a maximum number of hydrogen atoms in a lipid -> these lipids are solid at room temperature and are common in land animals

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29
Q

Unsaturated

A

If there is one carbon-carbon bound in a fatty acid -> these lipids are liquid at room temperature because of the carbon-carbon double bond -> most common in aquatic animals

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30
Q

What is more healthy saturated or unsaturated fats?

A

Unsaturated bonds

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31
Q

Polyunsatured

A

If there is more than one carbon carbon double-bond

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32
Q

Why do lipids not dissolve in water?

A

They are non polar

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33
Q

Nucleic Acids

A

(aka polynucleotides) macromolecules that store and transmit hereditary information

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34
Q

What are nucleic acids made of?

A

Contain hydrogen, oxygen, nitrogen, carbon, and phosphorus -> made from monomers called nucleotides (which in turn consists of three parts)

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35
Q

What are the three different parts of a nucleotide?

A

Phosphate Group, 5-carbon sugar, and nitrogenous base

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36
Q

How are nucleic acids formed?

A

when nucleotides covalently bond

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37
Q

How many types of nucleic acids are there?

A

2

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38
Q

What are the different types of nucleic acids?

A

RNA (ribonucleic acids) and DNA (deoxyribonucleic acids)

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39
Q

How are nucleic acids formed?

A

Through dehydration synthesis

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40
Q

What are the nitrogenous bonds held together by?

A

Hydrogen Bonds

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41
Q

Proteins

A

functional macromolecules that contain nitrogen, carbon, hydrogen, and oxygen (one of the most diverse kind of macromolecules)

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42
Q

What are proteins made of?

A

monomers -> amino acidsamino acids assembled into polypepdite chains

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43
Q

Amino Acids

A

compounds with an amino group (-NH2) on one end, a carboxyl group (-COOH) on the other end, a carbon atom in the center, a hydrogen atom on one side, and an R-group on the other

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44
Q

How are amino acids bonded together?

A

covalently bonded through bonds called pepdite bonds

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45
Q

Polypepdite

A

formed when MANY amino acids pepdite bond

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46
Q

What do proteins do?

A

Some proteins control the rate of reactions and regulate cell processes; others form important cellular structures; others transport substances into or out of cells to help or fight disease

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47
Q

More than ___ different amino acids are found in nature

A

20

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48
Q

Examples of amino acids found in nature

A

enzymes, hormones

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49
Q

How are the polypepdite chains in proteins assembled?

A

According to instructions in DNA

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50
Q

How many levels of organization does an amino acid have?

A

4

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51
Q

What are the levels of structure of an amino acid?

A

structure of an amino acid?

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52
Q

How many ways can polypepdite chains coil/fold and what are they?

A

in a zig-zag way and in curly way(look at notes)

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53
Q

The ___ of an amino acid always stays the same while the ___ changes

A

backbone (which consists of the carboxyl group, amino group, carbon atom, and hydogen atom); R-Group

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54
Q

All amino acids are identical except for at the ___

A

R -Group (which all are unique because they can be polar, nonpolar, acidic, basic, etc.)

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55
Q

What causes amino acids ability to bond?

A

Any amino acid can form to any carboxyl group because they are all the same

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56
Q

How are amino acids formed?

A

Through dehydration synthesis

57
Q

Dehydration Synthesis

A

to put together macromolecules by losing water. This is possible because by losing H20 you are linking two monomers together(look at model in notebook)

58
Q

Hydrolysis (Digestion)

A

to separate with the addition of water. This is possible because when water is added to a large organic molecule, one monomer will take the OH- and the other will take the H+, creating two monomers.

59
Q

Mass number

A

total number of protons and neutrons in nucleus

60
Q

Difference between deoxyribose and ribose

A

deoxy has one less oxygen molecule

61
Q

DNA bases

A

A G C T

62
Q

RNA bases

A

A G C U

63
Q

What is the main function of proteins?

A

they don’t have one

64
Q

Carbohydrates molecules

A

C H O

65
Q

Lipids molecules

A

C H O

66
Q

Proteins molecules

A

C H O N

67
Q

Nucleic Acids molecules

A

C H O N P

68
Q

Water chemical formula

A

H2O

69
Q

Water is a neutral molecule(True or False)

A

TRUE

70
Q

Polar Molecule

A

A molecule in which the charges are unevenly distributed;(Charges written parentheses (+) or (-) to show that the charges are weaker than ions) polar molecules attract each other because of their slight negative and positive charge

71
Q

Why are water molecules considered polar molecules?

A

Water molecules are considered polar molecules because they consist of one oxygen atom (that has a stronger pull because it has more protons in the nucleus) and two hydrogen atoms (which have a weaker pull because it has less protons in its nucleus) This causes the oxygen molecule to get more electrons than the hydrogen atoms in the covalent bond, causing the oxygen molecule to have a slightly negative charge and the hydrogen molecules to have a slightly positive charge.

72
Q

Hydrogen Bonding

A

Attraction of water molecules because of the slightly negative and positive charges of a water molecule; not as strong as covalent or ionic bonds (temporary)

73
Q

What are the most common atoms involved in hydrogen bonding?

A

Oxygen, nitrogen, and fluorine

74
Q

Cohesion

A

attraction between molecules of the same substance -> always through hydrogen bonds; creates a surface tension which allows some insects to walk on water(Ex:water molecules)

75
Q

Adhesion

A

attraction between molecules of different substances -> always through hydrogen bonds(Ex: water molecules and glass molecules)

76
Q

Capillary Action

A

One of the forces that draws water out of the roots of a plant and up into its stems and leaves. This is a combination of cohesion (which holds the water molecules together) and adhesion (which causes the water to rise)

77
Q

Heat Capacity

A

the amount of heat energy required to increase an object’s temperature

78
Q

Heat Capacity of Water

A

Water has a high temperature because it is highly cohesive. This means that the heat energy needs to break multiple hydrogen bonds before the heat spreads. (water needs to absorb more heat before it rises in temperature)

79
Q

Mixture

A

a material composed of two or more elements or compounds that are physically mixed together, but not chemically combined.

80
Q

Types of mixtures

A

Solutions and Suspensions

81
Q

Solution

A

a mixture in which all components are evenly distributed(Ex: salt dissolving in warm water)

82
Q

Suspension

A

mixtures of water and non dissolved material(Ex: our blood is mostly water and suspended cells)

83
Q

Solute

A

the substance that is dissolved

84
Q

Solvent

A

the substance in which the solute dissolves

85
Q

ph Scale

A

system used to indicate the concentration of H+ (hydrogen) ions in a solution. This system ranges from 0-14; below 7 the ph is acidic, at 7 the ph is neutral, above 7 the pH is basic.the pH scale is logarithmic meaning each step represents a factor of 10 difference

86
Q

Base

A

(aka proton acceptors) a compound that produces OH- (hydroxide) ions in a solution; pH above 7

87
Q

Why are bases known as proton acceptors?

A

Bases are known as proton acceptors because they attract H+ ions to create water.(look at example in notebook)

88
Q

Buffer

A

weak acids or bases that can react with strong acids or bases to prevent sharp, sudden change in pH. -> extremely important for maintaining homeostasis because enzymes can only operate under certain conditions

89
Q

Acid

A

(aka proton donors)any compound that forms H+ (hydrogen) ions in a solution -> compounds that are acidic are corrosive and break down other compounds; pH below 7

90
Q

Why are acids considered proton donors?

A

Acids are considered proton donors because they give off H+ ions. These hydrogen ions are considered protons because to become an ion they need to get rid of the one electron in there valence shell.

91
Q

One Universal Solvent

A

water

92
Q

What can water dissolve/Why is it known as a universal solvent?

A

ionic compounds, other polar molecules

93
Q

How does water dissolve compounds?

A

water molecules are attracted to positive/negative charge of other molecules (because of its bent shape) and pulls them apart, forming new compounds

94
Q

What does water expand upon freezing?

A

Because when water drops in temperature, the hydrogen bonds push the H20 molecules farther apart from each other increasing the intermolecular space, making it less dense than the water

95
Q

Atom

A

basic unit of matter; made of smaller subatomic particles

96
Q

Subatomic particles that make up an atom

A

Protons, neutrons, electrons

97
Q

What makes up an atom?

A

Nucleus, electrons, protons, neutrons, empty space, electron shells, valence

98
Q

Proton

A

positively charged particles

99
Q

Neutron

A

Particles with no charge

100
Q

What makes up the nucleus of an atom

A

Protons and neutrons

101
Q

What is the charge of an atom

A

neutral

102
Q

Strong nuclear force

A

for that holds the protons and neutrons in the nucleus of an atom together

103
Q

What takes up 99% of the mass of an atom

A

Nucleus

104
Q

Where is the nucleus of an atom located

A

center of an atom

105
Q

How do you measure the mass of the nucleus of an atom?

A

With atomic mass units (A.M.U) or daltons

106
Q

One proton/neutron are equal to?

A

1 AMU (or dalton)

107
Q

Electron

A

Negatively charged particle with 1/1840 mass of a proton. Electrons are in constant motion in the space surrounding the nucleus because they are attracted to the positive charge of the protons but do not bond with them because of their fast motion.

108
Q

There are ____ amount of protons and neutrons in the nucleus of an atom.

A

an even (usually)

109
Q

What is the charge of an (most) atom?

A

Neutral because they have an even amount of electrons and protons.

110
Q

Electron Cloud

A

the space in which the electrons are most likely to be around the nucleus. (This uncertainty of where the electrons will be are due to the Heisenberg uncertainty principle) fun fact :)

111
Q

Valence Shell

A

Outermost shell of an atom; contains valence electrons

112
Q

Electron shell vs Electron Cloud

A

Electron Shell - used to visualize where electrons are, and how many are on each levelElectron Clod - describes location and energy of electrons

113
Q

Element

A

pure substance that consists entirely of one type of atom.

114
Q

More than ___ elements are known but only about ____ are commonly found in living organisms

A

100; 24

115
Q

How are elements written?

A

One or two letter symbols (Na, H)

116
Q

Atomic Number

A

amount of protons in the nucleus; written bottom left

117
Q

Isotope

A

Elements with differing amounts of neutrons (Carbon-6, Carbon-7,etc.)(Elements can be isotopes of one another)

118
Q

Mass number

A

total amount of protons and neutrons (written top left)

119
Q

How are isotopes identified?

A

by their mass number

120
Q

Atomic mass

A

Average mass of all of the isotopes of a given element

121
Q

96% of living matter is made of __ elements:

A

4; nitrogen, oxygen, carbon, and hydrogen

122
Q

Radioactive Isotope

A

Isotopes that have a radioactive nuclei, which break down over time because they have a very different amount of neutrons from the original amount

123
Q

Uses of radioactive isotopes

A

Can be dangerous, but also used to treat cancer, determine the age of rocks and fossils, kill bacteria, etc.

124
Q

Compound

A

a substance formed by the chemical combination of two or more elements, in the same (never changes) proportions

125
Q

Chemical Formula

A

shows the composition of compounds (H20, NaCl)

126
Q

Chemical Bonds

A

bonds that hold the atoms in compounds together. Formed with the valence electrons

127
Q

Main types of Chemical Bonds

A

ionic bonds, covalent bonds, hydrogen bonds

128
Q

Ionic Bonds

A

formed when one or more electrons are transferred from one atom to another.(because one atom has too many valence electrons and needs to give away to get 8 -> gives to atom with less than 8 valence electrons)

129
Q

Covalent Bonds

A

formed when electrons are shared by atoms.(because both electrons need 8 valence electrons but not give any away)

130
Q

Ion

A

positively or negatively charged atoms

131
Q

molecule

A

the smallest unit of most compounds; formed when atoms covalently bond

132
Q

Van der Waals Forces

A

When atoms covalently bond to form molecules there is sometimes a charge that forms, (positive or negative) because one atom might have a stronger pull on the electrons being shared than the other atom. This causes molecules to be attracted to one another (if one positive and other negative). This INTERMOLECULAR force is extremely weak.

133
Q

Octet Rule

A

Atoms always want an outer layer of 8 valence atoms (reason for bonds)

134
Q

Single Bond

A

2 shared electrons

135
Q

Double Bond

A

4 shared electrons

136
Q

Triple bond

A

6 shared electrons

137
Q

Important Chemical Formulas

A

Glucose; Water

138
Q

Water

A

H20

139
Q

Glucose

A

C6H1206

Bio HO9 (11 decks)

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