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Biology 107 POWERPOINT SLIDES > Chapter 2- Matter > Flashcards

Chapter 2- Matter Flashcards

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1
Q

What is matter?

A

Anything that has mass and occupies space.

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2
Q

What are 2 types pure substances?

A

Elements

Compounds

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3
Q

What are the two classifications of matter?

A

Pure substances

Mixtures

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4
Q

What are the two types of mixtures?

A

Heterogenous

Homogenous (solutions)

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5
Q

What is an element?

A

A pure substance which cannot be broken down into anything simpler via physical or chemical means

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6
Q

What is a compound?

A

A pure substance that can be decomposed by a chemical change into simpler substance with a fixed mass ratio

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7
Q

What is an example of heterogenous mixtures?

A

Salt and Pepper

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8
Q

What is an example of homogenous mixtures?

A

Kool-Aid

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9
Q

Even with its vast diversity, all life is based upon ________.

A

A limited number of chemical elements

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10
Q

What elements comprise the human body?

A 
Oxygen (O) - 65%
Carbon (C) - 18.5%
Hydrogen (H) - 9.5%
Nitrogen (N) - 3.3%
Calcium (Ca) - 1.5%
Phosphorous (P) - 1.0%
Potassium (K) - 0.4%
Sulfur (S) - 0.3%
Sodium (Na) - 0.2%
Chlorine (Cl) - 0.2%
Magnesium (Mg) - 0.1%
Trace Elements - <0.01%
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11
Q

Every element is composed of _______.

A

Atoms

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12
Q

Atoms of a given element are ______.

A

Identical

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13
Q

Atoms of an element are _________ into atoms of another element by chemical processes.

A

Not changed

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14
Q

Where are protons and neutrons locates?

A

In the nucleus of an atom

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15
Q

Where are electrons located?

A

Orbiting in energy levels around the nucleus of an atom

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16
Q

A proton has a _________ charge.

A

Positive

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17
Q

An electron has a _________ charge.

A

Negative

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18
Q

A neutron has _________ charge.

A

No

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19
Q

What is the unit of measure for an atom?

A

amu

Atomic Mass Unit

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20
Q

1 amu = _______.

A

The mass of one proton

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21
Q

How much smaller are electrons than 1 amu?

A

Almost 2,000 times smaller.

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22
Q

Do any elements have the same number of protons?

A

No

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23
Q

Atomic number =

A

Number of protons =

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24
Q

What is the mass number?

A

Protons + Neutrons

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25
Q

Isotopes are comprised of what?

A

Same # protons, different # neutrons

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26
Q

What is the atomic mass or weight?

A

The average mass of the atoms of an element

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27
Q

What is the atomic mass of Carbon (C)?

A

12.011 amu

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28
Q

What can radioactive isotopes be used for?

A

Diagnostic medicine

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29
Q

Radioactive compounds in metabolic processes act as what?

A

Tracers

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30
Q

How can radioactive isotopes be traced in living organisms?

A

Through instruments designed to detect the radioactive isotopes

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31
Q

Are radioactive isotopes harmful to us?

A

Yes

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32
Q

Uncontrolled radioactive isotope exposure can lead to what?

A

Damage to some molecules in a living cell (cellular molecules) especially DNA

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33
Q

Chemical bonds are broken by radioactive isotopes causing what?

A

Abnormal bonds

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34
Q

How are elements arranged on the Periodic Table of Elements?

A

Left to right, top to bottom in order of increasing atomic number

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35
Q

In the table of elements, what is a row called?

A

A period

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36
Q

In the table of elements, what is a column called?

A

A group

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37
Q

What determines an atom’s chemical properties?

A

The distribution of electrons around the nucleus

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38
Q

Where exactly are electrons located?

A

In the electron shield

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39
Q

How many electrons can the 1st electron shell hold?

A

2

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40
Q

How many electrons can the second shell hold?

A

8

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41
Q

How many electrons can the 3rd shell hold?

A

18

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42
Q

When is an electron shell considered full?

A

When it contains 8 electrons

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43
Q

What is the formula for determine the electron amount per shell?

A

2(n)^2

N=shell number

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44
Q

How many electron shells may an atom have?

A

1-7 electron shells

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45
Q

What is the outermost electron shell called?

A

The Valence shell

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46
Q

What determines the chemical properties of an atom?

A

The number of electrons in the outermost (valence) shell

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47
Q

What may occur to atoms who’s valence shell is not full?

A

They interact with other atoms in ways that enable them to complete or fill their valence shell

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48
Q

What is the OCTET rule?

A

Atoms tend to gain, lose, or share electrons so as to have 8 electrons

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49
Q

What are compounds?

A

Two or more elements chemically combined to form a new substance with new properties

50
Q

Is sugar a compound or element?

A

Compound

51
Q

What is one of the simpler substances sugar can be broken down into?

A

Carbon (the black element created).

52
Q

Can Carbon be broken down into a simpler element? Why?

A

No. Carbon is an element and cannot be further decomposed by chemical or physical means.

53
Q

What is a radioactive isotope?

A

One in which the nucleus decays spontaneously, giving off particles and energy.

54
Q

When a neutral atom loses an electron (-), it becomes a __________ with what kind of charge?

A

Cation (+)

55
Q

When a neutral atom gains an electron (-), it becomes a __________ with what kind of charge?

A

Anion (-)

56
Q

What are covalent bonds?

A

When atoms share more than 2 valence electrons.

57
Q

How many electrons are share in a double covalent bond?

A

4 electrons are shared

58
Q

How many electrons are shared in a triple covalent bond?

A

6 electrons are shared.

59
Q

How many electrons are shared in a covalent bond?

A

2 electrons are shared.

60
Q

Chemical reactions do what to chemical bonds?

A

Make or break chemical bonds

61
Q

What is a reactant?

A

The compounds exposed to a chemical reaction

62
Q

What is the end result of a chemical reaction called?

A

Product(s)

63
Q

Matter neither is created nor destroyed, so what occurs to

(2)H2 + O2 when it reacts?

A

(2)H20

64
Q

What are molecules?

A

Combinations of atoms held together by covalent bonds to form compounds
(H20)

65
Q

What is electronegativity?

A

The atom’s affinity for electrons

66
Q

What dictates how electrons are distributed in a covalent bond?

A

Differences in electronegativity

67
Q

What are nonpolar covalent bonds?

A

Equal sharing of electrons

68
Q

What are polar covalent bonds?

A

Unequal sharing of electrons

69
Q

Why is H20 a polar covalent bond?

A

Because the atoms are not sharing electrons evenly

70
Q

Why is one side of water negatively charged?

A

Because the oxygen atom keeps the electrons longer than the hydrogen atoms, creating a negative charge.

71
Q

The oxygen side of water charged how?

A

Positively charged

72
Q

What are the 7 properties of water?

A
  1. Adhesion
  2. Cohesion
  3. Capillary action
  4. High surface tension
  5. Holds heat to regulate temperature (high heat capacity
  6. Less dense as a solid than a liquid
  7. Universal solvent
73
Q

Water is Adhesive to what type of molecules?

A

Any substance it can form hydrogen bonds with

74
Q

What does adhesion refer to?

A

Attraction to other polar substances

75
Q

What property is related to cohesion?

A

Surface tension

76
Q

What does cohesion refer to?

A

It refers to attraction to other water molecules (like molecules)

77
Q

What is surface tension?

A

The measure of the force necessary to stretch or break the surface of a liquid.

78
Q

Surface tensions makes water behaves as if….

A

It were covered by an invisible film

79
Q

Due to surface tension, what can some animals do on water?

A

Stand, walk, or run without breaking the surface

80
Q

When is capillary action present?

A

When a molecules has both adhesive and cohesive attributes

81
Q

What is capillary action? (H20)

A

Water is attracted to another material (adhesion) and through COHESION other water molecules move too as a result of the original cohesion

82
Q

Flubber is an example of ….

A

Capillary action 😂

83
Q

Water has a high specific heat. What does that mean?

A

A very high temperature is required to changes the molecules’ temperature (H2O)

84
Q

Water has a high heat of vaporization. What is a result of vaporization?

A

The evaporation of water from a surface causes cooling of that surface (evaporative cooling)

85
Q

Each water molecule can form up to ______ with neighboring water molecules

A

4 H-bonds

86
Q

What occurs to H bonds of water in a liquid state?

A

They are constantly formed and broken

87
Q

Why does water have a high melting/boiling point?

A

Because it requires a lot of thermal energy (heat) to break the H bonds of water

88
Q

Why is water less dense as a solid than a liquid?

A

Because the molecules are spread further than a liquid

89
Q

Hydrogen bonds in ice are stable/unstable?

A

Stable

90
Q

The Hydrogen Bonds in liquid water are stable/unstable?

A

Unstable

91
Q

Why is water a solvent?

A

It dissolves salts by forming a shell of interacting water molecules around the ions. This weakens the electrostatic interactions between the ions

92
Q

Because unlike charges attract, the negative end of water (H2O) will be attracted to ________ .

A

The positive end of salt, Na(+).

93
Q

Because unlike charges attract, the positive end of water (H2O) will be attracted to ________ .

A

The negative end of Salt: the negative chloride ion, Cl (-)

94
Q

Once water attaches to salt, what occurs?

A

Due to the fluid nature of water, it pulls upon the ionic compound of salt (Na- Cl+) until their ionic bond is broken and the ionic molecules move away from from each other (dissolving)

95
Q

What is a solution?

A

A mixture of two or more substances in a single phase

96
Q

What are the two TYPES of substances in a mixture?

A

1 solvent

2+ solutes

97
Q

What types of molecules can form H-bonds with water?

A

Polar molecules with electronegative atoms

98
Q

What are hydrophilic compounds?

A

Compounds that easily dissolve in water

99
Q

Hydrophilic comes from the Greek “?”

A

“Water-loving”

100
Q

What are hydrophobic compounds?

A

Compounds that do no readily dissolve in water

101
Q

Hydrophobic means “?”

A

“Water-hating”

102
Q

Why does oil and water not mix?

A

Oil is non polar
Water is polar

Only polar compounds can form bonds with H20

103
Q

Because water is an cohesive molecule, explain why oil and water do not mix.

A

Water is attracted to itself through its polar negativity (cohesion). Oil has no polar negativity. Water will attempt to join like molecules, push the non-polar molecules out of the way in.

104
Q

In LIQUID water, a small percentage of water molecules break apart into what?

A

Ions

105
Q

What ions are produced in liquid water?

A 
Hydrogen ions (H+)
Hydroxide ions (OH-)
106
Q

Ionizing a water molecule (H2O) results in what?

A

(H+) + (OH-)

Hydrogen ion + hydroxide ion

107
Q

Hydrogen and hydroxide ions are very __________.

A

Reactive

108
Q

What is an acid?

A

A substance that produces H+ ions when dissolved in water (hydrogen ions increase)

109
Q

What is a base?

A

A substance that produces OH- ions when dissolved in water

110
Q

What is the pH scale?

A

A scale describing how acidic or basic a solution is

111
Q

What is the range of the pH scale?

A

Most Acidic (0)

to

Most Basic (14)

112
Q

What does each unit of the pH scale represent?

A

Each pH units represents a 10-fold change in the H+ concentration in a solution

113
Q

Name a few examples of base, neutral, and acidic solutions.

A

Base- (.5) battery acid, lemon juice, gastric juice

Neutral- human urine, saliva, pure water, human blood, tears, seawater

Acid- (13) oven cleaner, (11) household bleach, household ammonia

114
Q

What is a buffer?

A

A substance that minimizes changes in pH

115
Q

What do buffers do chemically?

A
  • Accept H+ ions when in excess

- Donate H+ ions when depleted

116
Q

The chemistry of life is sensitive to what?

A

Acidic and basic conditions

117
Q

What are isotopes?

A

One of several forms of an element, each with the same number of protons, but different number of neutrons.

118
Q

What are groups specifically?

A

Elements in a vertical column have the same number of electrons in their valence shell

119
Q

What do elements of a group share?

A

Chemical properties

120
Q

What is a period of The Periodic Table, specifically.

A

Each horizontal row contains elements with the same total number of electron shells.
Across each period, elements are ordered in increasing atomic number.

121
Q

How does evaporative cooling occur?

A

Molecules with the greatest energy leave (evaporate) thus lowering the temperature of remaining molecules allowing for heat to leave while the surface remains cool.

Biology 107 POWERPOINT SLIDES (9 decks)

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