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Principles of Biology 103 > Chapter 2 (Exam One) > Flashcards

Chapter 2 (Exam One) Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Matter?

A

refers to anything that has mass and occupies space.

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2
Q

Matter exists in three states:

A

solid, liquid, gas

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3
Q

All matter (both living and non-living) is composed of?

A

Basic substances called elements

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4
Q

A element is?

A

a substance that cannot be broken down into substances with different properties; composed of one type of atom.

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5
Q

How many elements are naturally occurring?

A

92

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6
Q

6 elements makeup 95% of the body weight of organisms, what are they?

A 
(CHNOPS)
Carbon
Hydrogen
Nitrogen
Oxygen
Phosphorus
Sulfer
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7
Q

A atom is?

A

the smallest part of an element that displays the property of the element.

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8
Q

A atom is composed of?

A

Protons, neutrons, electrons, and a central nucleus

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9
Q

proton?

A

Positively charged, 1 amu

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10
Q

Neutron?

A

No charge, 1 amu

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11
Q

Electron?

A

Negatively charged, very low mass-negligible in calculations

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12
Q

Electron shells?

A

Orbiting clouds around the nucleus

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13
Q

Each element is represented by?

A

One or two letters to give it a unique s=ymbol

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14
Q

H?

A

Hydrogen

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15
Q

Na?

A

Sodium

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16
Q

C?

A

Carbon

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17
Q

The atomic number is?

A

Equal to the number of protons in each atom of an element

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18
Q

The mass number? Atomic mass

A

Of an atom is equal to the sum of the number of protons and neutrons in atoms nucleus

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19
Q

The atomic mass?

A

Is approximately equal to the mass number

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20
Q

Periods?

A

Atoms of an element arranged horizontally by increasing atomic number in rows

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21
Q

Groups?

A

Atoms of an element arranged in vertical columns

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22
Q

Atoms shown in the the periodic table are?

A

Electrically neutral

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23
Q

The atom number tell you’d the number of ______ as well as the number of _____?

A

Electrons, protons

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24
Q

Isotopes?

A

Are atoms of the same element that differ in the number of neutrons (and therefore different atomic masses.)

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25
Q

Some isotopes spontaneously?

A

Decay

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26
Q

Radioactive isotopes?

A

Give off energy in the form of rays and subatomic particles

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27
Q

Carbon 14 is an example of? What’s is been used for?

A

A radioactive isotope; been used to examine reactions in photosynthesis

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28
Q

Isotopes can be?

A

Helpful or harmful

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29
Q

Electrons are attracted to?

A

The positively charged nucleus; thus it takes energetically to hold electrons in place

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30
Q

What does it take to push elections away?

A

It takes energy to push them away and keep them in their own shell

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31
Q

The more distant the shell?

A

The more energy it takes to hold in place

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32
Q

Elections determine?

A

Chemical behavior of atoms

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33
Q

Bohr model?

A

Is a useful way to visualize electron location

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34
Q

Another word for Energy levels?

A

Energy shells

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35
Q

Electrons revolve around? In what form?

A

The nucleus; in energy shells

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36
Q

The following rules apply for atoms with atomic numbers of 20 or less?

A
  • The first energy shell can hold up to 2 electrons
  • Each additional shell can hold up to 8 electrons
  • Each lower shell is filled first before electrons are placed in the next shell
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37
Q

Valence shell?

A

The outermost energy shell of any atom

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38
Q

The valence shell is important because?

A

It determines many of an atoms chemical properties

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39
Q

Octet rule?

What’s the one exception?

A

States that the outermost shell is most stable when it has 8 electrons
Exception: if an atom has only one shell, the outermost valence shell is complete when it has two electrons

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40
Q

Chemical reaction?

A

The process of bond formation

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41
Q

Ion?

A

Is an atom that has lost or gained an electron

42
Q

Ionic bond? Example

A

Forms when electrons are transferred from one atom to another atoms and the oppositely charged ions are attracted to each other
Formation of sodium chloride

43
Q

Salts?

A

Are solid substances that usually separate and exist as individual ions in water

44
Q

Covalent bonds?

A

Result when two atoms share electrons so each atom has an octet of electrons in the outer shell

45
Q

Nonpolar covalent bond? Examples

A

Electrons are shared equally between atoms

Hydrogen gas, oxygen gas, methane

46
Q

Polar covalent bond? Example?

A

Electrons are shared unequally

Water

47
Q

Electronegativity?

A

Is the ability of an atom to attract electrons towards itself in a chemical bond

48
Q

Water is a?

A

Polar molecule

49
Q

Hydrogen bond?

A

Is a weak attraction between a slightly positive hydrogen atom and a slightly negative atom

50
Q

Water molecules cling together because of?

A

Hydrogen bonding

51
Q

_____ has a high heat capacity?

A

Water

52
Q

The presence of many hydrogen bonds allow?

A

Water or absorb a large amount of thermal energy without a great change in temperature

53
Q

The temperature of water?

A

Rises and falls slowly

54
Q

Water has a high heat of?

A

Evaporation

55
Q

Hydrogen bonds must be?

A

Broken to evaporate water

56
Q

Bodies of organisms?

A

Cool when their heat is used to evaporate water

57
Q

Water is a good?

A

Solvent

58
Q

Why is water a good solvent?

A

Because of its polarity

59
Q

Polar substances?

A

Dissolve readily in water

60
Q

Hydrophilic?

A

Molecules dissolve in water

61
Q

Hydrophobic?

A

Molecules do not dissolve in water

62
Q

Solution?

A

Contain dissolved substances or solutes

63
Q

Water molecules are?

A

Cohesive and adhesive

64
Q

Cohesion?

A

Is the ability of water molecules to cling to each other due to hydrogen bonding

  • water flows freely
  • surface tension
65
Q

Adhesion?

A

Is the ability of water molecules to cling to other polar surfaces

  • due to waters polarity
  • capillary action
66
Q

Cohesion and adhesion account for?

A

Water transport in plants as well as transport in blood vessels

67
Q

Frozen water (ice) is?

A

Less dense than liquid water

68
Q

Water expands as it?

A

Reaches 0c and freezes

69
Q

Ice floats? It acts as what while doing this?

A

On liquid water ; acts like an insulator on top of a frozen body of water

70
Q

pH?

A

Is a measure of hydrogen ion concentration in a solution

71
Q

When water ionizes and dissociate, it?

A

Releases an equal number of hydrogen (H+) ions and hydroxide (OH-) ions

72
Q

Acids?

A

Are substances that dissociate in water releasing hydrogen ions

73
Q

Bases?

A

Are substances that either take up hydrogen ions or release hydroxide ions

74
Q

pH scale?

A

Is used to indicate the acidity or basicity (alkalinity) of a solution

75
Q

0 to <7 =

A

Acidic

76
Q

7 =

A

Neutral

77
Q

> 7 to 14 =

A

Basic (or alkaline)

78
Q

Logarithmic scale?

A

Each unit change in pH represents a 10-fold change in H+ concentration

79
Q

Buffer?

A

Is a chemical or a combination of chemicals that keeps pH within normal limits

80
Q

Human blood is normally pH?

A

7.4 (slightly basic)

81
Q

Acidosis?

A

If blood pH drops below 7.0

82
Q

Alkalosis?

A

If blood pH rises above 7.8

83
Q

An element and atom share what?

A

the same name

84
Q

Atoms within the same group share what?

A

the same chemical binding characteristics

85
Q

Electrons have energy due to what? What’s the energy called?

A

Relative position; potential energy

86
Q

The number of electrons in an atom’s valence shell determines what?

A

Whether the atom gives up, accepts, or shares electrons to acquire eight electrons in the outer shell

87
Q

Atoms that have their valence shells filled with electrons tend to what?

A

Be chemically stable

88
Q

Atoms that do not have their valence shells filled with electrons are what?

A

Chemically reactive

89
Q

A molecule is what?

A

Two or more elements bonded together. Smallest part of a compound that retains its chemical properties

90
Q

A compound is what?

A

A molecule containing at least two different elements bonded together.

91
Q

A formula tells what

A

The number of each kind of atom in a molecule

92
Q

Bonds that exist between atoms in molecules contain what?

A

Energy

93
Q

Bonds between atoms are caused by what?

A

The interactions between electrons in outermost energy shells

94
Q

What makes hydrogen bonding possible in water? What’s this an example of?

A

The shape of a water molecule and its polarity. Structure-function relationship

95
Q

A hydrogen bond can occur between what?

A

Atoms of different molecules or with the same molecule

96
Q

A single hydrogen bond is what while multiple hydrogen bonds are what

A

Weak; strong

97
Q

A hydrogen bond helps to maintain what?

A

Proper structure and function of complex molecules such as proteins and DNA

98
Q

The temp of water rises and falls slowly and this allows organisms to what?

A

Maintain their normal internal temperatures, protected from rapid temperature changes

99
Q

At temperatures below what? Hydrogen bonds become what?

A

4 degrees Celsius. As they become more rigid but also more open

100
Q

Body has built in mechanisms to prevent pH changes. Example?

A

Carbonic avid buffer dissociates and reforms to reduce changes in pH

Principles of Biology 103 (14 decks)

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