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Intro to Bio > Bio Lecture Slides Series 2 (Chemistry of Life) > Flashcards

Bio Lecture Slides Series 2 (Chemistry of Life) Flashcards

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Biology 101 flashcards
1
Q

What are the two known components of the universe?

A

energy and matter

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2
Q

Define energy.

A

ability to do work, no mass, no volume; neither created nor destroyed, only changes form

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3
Q

Define matter.

A

has mass and occupies volume; neither created nor destroyed, only changes form.

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4
Q

What does E=MC2 tell us about matter and energy?

A

the formula reveals that energy and matter are related

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5
Q

Matter can exist as a _____, _____, or _____.

A

solid, liquid, or gas

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6
Q

Matter is composed of _____.

A

elements.

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7
Q

Define element.

A

a substance that cannot be broken down into another substance by ordinary chemical means

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8
Q

How many naturally occurring elements are there?

A

92

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9
Q

How many elements make up about 98% of the body weight of most organisms?

A

Six, CHNOPS (Carbon, Hydrogen, Nitrogen Oxygen, Phosphorus, Sulfur)

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10
Q

Name the elements in CHNOPS.

A

Carbon, Hydrogen, Nitrogen Oxygen, Phosphorus, Sulfur

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11
Q

In living organisms, the top two elements present are _____ and _____.

A

oxygen (65%) and carbon (18%)

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12
Q

In living organisms, the fewest occurring elements present are _____, _____, _____, and _____.

A

NCPS (nitrogen, calcium, phosphorus, sulfur)

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13
Q

Atomic theory states that elements consist of _____.

A

atoms

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14
Q

Define atom.

A

the basic unit of matter

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15
Q

Define atomic symbol.

A

name of the atom or element

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16
Q

Name the three subatomic particles.

A

neutrons, protons, electrons

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17
Q

Describe a neutron.

A

no electrical charge, found in nucleus

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18
Q

Describe a proton.

A

positive charge, found in nucleus

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19
Q

Describe electrons.

A

negative charge, found outside of nucleus

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20
Q

Mass number is equal to the ____________.

A

sum of protons and neutrons – electrons have about zero mass

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21
Q

Atomic weight changes with _____.

A

gravity

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22
Q

All atoms of an element have the _____ number of protons.

A

same

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23
Q

The atomic number also gives number of _____ if an atom is electrically neutral.

A

electrons

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24
Q

In the periodic table, the chemical elements are arranged in order of _____ _____ _____.

A

increasing atomic number

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25
Q

In the periodic table, the rows are called _____.

A

periods

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26
Q

In the periodic table, the columns are called _____.

A

groups

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27
Q

Elements’ chemical and physical characteristics recur in a _____ manner on the periodic table.

A

predictable

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28
Q

On the periodic table, atoms are arranged in _____ and _____.

A

periods (rows) and groups (columns)

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29
Q

Variations of atoms are called _____ and _____.

A

ions and isotopes

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30
Q

Ions are __________.

A

atoms or small molecules that have gained or lost an electron

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31
Q

Isotopes are __________.

A

elements with same number of protons but different numbers of neutrons

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32
Q

Isotopes have naturally occurring variations in the number of _____.

A

neutrons

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33
Q

The imbalance between the numbers of protons vs. electrons creates the charged particle known as a(n) _____.

A

ion

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34
Q

Are isotopes stable or unstable?

A

unstable

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35
Q

Do isotopes emit radiation?

A

Yes, the more unstable they become and the more decay

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36
Q

Define half life.

A

The amount of time it takes for half the mass of a radioactive isotope to breakdown

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37
Q

Radioactive isotope behavior is essentially the same as a stable isotope of the same element. True or false?

A

True

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38
Q

Isotopes can be used as tracers in PET scans. True or false?

A

True

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39
Q

Isotopes can cause damage to cells leading to cancer. True or false?

A

True

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40
Q

Isotopes can be used to sterilize medical equipment. True or false?

A

True

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41
Q

Isotopes Can be used to date very old objects. True or false?

A

Can be used to date very old objects

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42
Q

Do electrons have much mass?

A

No they do not, they have a mass of 9.1 x 10-28

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43
Q

The electrical charge (while opposite) of an electron is _____ that of a proton.

A

equal to

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44
Q

Where are electrons found?

A

Electrons are found outside the nucleus (most of the atom being empty space) in energy levels called shells.

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45
Q

Electrons move in some fashion _____ the nucleus.

A

around

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46
Q

Changes in the nucleus of an atom are called _____ _____.

A

nuclear reactions (rxn)

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47
Q

Electrons are responsible for all chemical reactivity because __________.

A

they are always changing

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48
Q

Electrons are attracted to the __________.

A

positively charged nucleus

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49
Q

Inner shell electrons require _____ energy to stay in the atom than electrons further from the nucleus.

A

less

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50
Q

Electrons are associated with certain energy levels because __________.

A

electrons are attracted to the positively charged nucleus, and inner shell electrons require less energy to stay in the atom than electrons further from the nucleus.

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51
Q

The energy of an electron can be expressed as a _____ _____ _____.

A

Frequency of light. Electrons have the ability to absorb certain wavelengths or frequencies of light.

52
Q

Once electrons absorb energy they jump up to a new electron shell (at a higher E level). True or false?

A

True.

53
Q

Because _____ are limited to an energy level within the atom, they cannot hold on to this energy and fall back to their shell and give back off the E they absorbed.

A

electrons

54
Q

This ability of electrons are important to biological processes _____ and _____ and the principle is applied to produce fluorescent lights.

A

photosynthesis, respiration

55
Q

According to fill order, the first electron shell can hold up to _____ electrons.

A

2

56
Q

According to fill order, the second electron shell can hold up to _____ electrons.

A

8

57
Q

According to fill order, the third electron shell can hold up to _____ electrons.

A

18

58
Q

According to fill order, the fourth electron shell can hold up to _____ electrons.

A

32

59
Q

According to fill order, third and fourth shells will not fill with more than 8 electrons until all _____ electrons are available

A

18 or 32

60
Q

Outer shell electrons called _____ _____ electrons and are responsible for chemical reactivity

A

valence shell

61
Q

A molecule is _____ or more atoms bonded together.

A

2

62
Q

Compounds contain more than one type of atom bonded together. True or false?

A

True

63
Q

Define Octet Rule.

A

All shells except the first are satisfied at 8 e- and bond to attain this more stable configuration.

64
Q

Name the three types of chemical bonding.

A

ionic, covalent, metallic

65
Q

An e- transfer that creates ions, one positive and one negative, and this electrostatic force holds the atoms together. It also occurs between metals and nonmetals and is called _____ bonding.

A

ionic bonding

66
Q

How does sodium behave in an ionic bond?

A

Sodium has 1 electron in valence shell and usually gives up an electron

67
Q

How does chlorine behave in an ionic bond?

A

Chlorine has 7 electrons in valence shell and usually accepts an electron from another atom

68
Q

Covalent bonding is essentially electron _____.

A

sharing

69
Q

In this type of bonding, each atom contributes one electron to make a pair and the force of attraction of each nuclei for this pair holds the atoms together in a bond.

A

covalent bonding

70
Q

Covalent bonds occur between two or more _____.

A

nonmetals, and more than one pair can be shared

71
Q

In covalent bonds, all molecules do not share equally – the greater the center of positive charge (nucleus) the more it can draw electrons in closer. True or false?

A

true

72
Q

Define polar covalent bond.

A

Two atoms are bonded and their nucleus contains different numbers of protons. All bonds except two of the same atoms are polar bonds.

73
Q

Picture 2 hydrogen atoms covalently bonded and sharing electrons to fill their first shell. How is this possible?

A

orbitals overlap

74
Q

Covalently bonded atoms may also share more than one pair of electrons, true or false?

A

True. A double bond = 2 pairs of e- shared. •A triple bond = 3 pairs of e- are shared.

75
Q

In which type of bond might a single atom form bonds with more than one atom?

A

covalent bond

76
Q

When atoms do not share the electrons equally this can also create molecules with an unequal distribution of charge. This is called a _____.

A

dipole (water is an example of a dipole)

77
Q

A molecule can contain polar bonds but not be a dipole. Which gas is an example of this?

A

methane

78
Q

Metallic bonding is essentially _____ _____.

A

electron pooling

79
Q

Which type of bond results in none of the valence e- belong to any one nucleus but are instead shared by all the nearby nuclei; occurs between 1, 2, or more metals?

A

metallic bond

80
Q

Which type of bond affects the properties of metals (i.e. shiny or metallic luster), the malleability of metal, and also responsible for the fact that most metals are great conductors of heat and electricity?

A

metallic bond

81
Q

A molecule used within the biochemical pathways of cells that has lost an electron and therefore will steal an electron from the closest molecule is known as a _____ _____.

A

free radical

82
Q

_____ _____ can set off a chain reaction resulting in cell death and even tissue damage.

A

Free radicals

83
Q

_____ _____ _____ is the latest theory to explain aging and some disease processes like cancer.

A

Free radical formation

84
Q

Scientist tell us the answer to free radicals are _____ any molecule that reacts with free radicals, neutralizing their ability to damage biological molecules.

A

antioxidants

85
Q

Well documented are: Vitamins C, D, E and beta carotene are well-documented _____ _____.

A

Dietary antioxidants

86
Q

Long term lack of vitamin _____ is associated with 15 types of cancer, including prostrate cancer in men.

A

D

87
Q

The latest antioxidants to be discovered are a group of _____ compounds, sometimes simply called phytochemicals.

A

plant

88
Q

Approximately 200 of phytochemical compounds have been identified to date and most are associated with _____ and _____.

A

fruits and vegetables

89
Q

Antioxidants are also anti-carcinogenic, which means they __________.

A

fight or prevent cancer

90
Q

In a chemical reaction, reactants are __________.

A

molecules that participate in reactions and are shown to the left of the arrow

91
Q

In a chemical reaction, products are __________.

A

molecules formed by reactions and are shown to the right of the arrow

92
Q

An equation is balanced when __________.

A

the same number of each type of atom occurs on both sides of the arrow because matter never disappears

93
Q

In chemical reactions, the two-way arrow means __________.

A

the rxn is reversible

94
Q

If a reaction is _____ it means that the initial or some of the initial reactants are regenerated at the end of the reaction so the reaction continues to occur.

A

cyclic

95
Q

All life began in _____.

A

water

96
Q

_____ is the single most important molecule on Earth.

A

water

97
Q

All organisms are 70-___% water.

A

90

98
Q

What type of bond is water?

A

polar covalent

99
Q

Which bond is a slightly positive hydrogen of one water molecule attracted to the slightly negative oxygen in another water molecule?

A

hydrogen bond

100
Q

Polar covalent bonds do not always result in a polar molecule, true or false?

A

true. (methane is an example)

101
Q

In a polar covalent bond, atoms do not share _____ equally.

A

electrons

102
Q

These properties (solvency, cohesion and adhesion, high surface tension, high heat capacity, high heat of vaporization, high heat of fusion, and varying density) all belong to which compound?

A

water

103
Q

Water is a compound and a _____.

A

solvent; it dissolves many substances

104
Q

Define hydrophilic.

A

molecules attracted to water

105
Q

Define hydrophobic.

A

molecules not attracted to water

106
Q

Water causes salt to _____.

A

dissociate

107
Q

The ability of water molecules to cling to each other due to hydrogen bonding is called _____.

A

cohesion

108
Q

The ability of water molecules to cling to other polar surfaces is called _____.

A

adhesion

109
Q

Adhesion and cohesion allow water to be an excellent _____ system inside and outside of living organisms.

A

transport

110
Q

High surface tension, how water molecules at the surface cling more tightly to each other than to the air above, is due to which bond?

A

hydrogen bond

111
Q

The many hydrogen bonds linking water molecules together allow water to absorb heat without greatly changing its temperature. This is the reason for water’s _____ _____ _____.

A

High heat capacity

112
Q

Temperature of water rises and falls slowly; this means that water _____ temperature.

A

stabilizes

113
Q

The following characteristics all relate to which property of water? Takes a great deal of energy to break H bonds for evaporation, heat is dispelled as water evaporates, high temperatures may damage enzymes.

A

high heat of vaporization

114
Q

Your sweating and water boiling are examples of which property of water?

A

high heat of vaporization

115
Q

Heat of _____ is the opposite of heat of vaporization.

A

fusion

116
Q

The amount of heat energy that must withdraw to cause water to freeze or change from liquid to solid.

A

heat of fusion

117
Q

Water’s _____ causes water molecules to align a particular way which results in air spaces, hence, solid water is less dense than liquid water. Also accounts for interesting formations like ice crystals and snow flakes.

A

polarity

118
Q

Liquid water is more _____ than ice.

A

dense, because unlike other substances, water expands as it freezes, ice floats rather than sinks, it makes life possible in water, and ice acts as an insulator.

119
Q

Water _____ into an equal number of hydrogen ions (H+) and hydroxide ions (OH-).

A

dissociates

120
Q

The mathematical way to indicate the number of hydrogen ions in solution is called _____.

A

pH

121
Q

The pH scale ranges from __________.

A

0 to 14; pH below 7 is acidic – more [H+] than [OH-]; pH above 7 is basic – more [OH-]than [H+]; pH of 7 is neutral – [H+] equal to [OH-].

122
Q

Pure water has a pH of _____.

A

7

123
Q

A _____ is a compound that accepts H+ in response to a pH change.

A

buffer

124
Q

_____ are chemicals or combination of chemicals keeps pH within normal limits.

A

buffers

125
Q

Buffers resist pH change by __________.

A

taking up excess H+ or OH-

126
Q

Blood has a neutral pH. True or false?

A

False. pH of blood is about 7.4 – maintained by buffers – the main one is the bicarbonate ion. If the blood becomes too acidic, bicarbonate accepts (and absorbs) H+ to make carbonic acid.

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