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currycurry UNIT ! > Chapter 2 Part 1 Lecture > Flashcards

Chapter 2 Part 1 Lecture Flashcards

1
Q

Purpose of Ch. 2: (4)

A
  • Introduce the language and fundamental concepts of chemistry
  • Discuss how matter is organized
  • Discuss how chemical bonds form and how chemical reactions occur
  • Compare and contrast organic and inorganic compounds
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2
Q

3 basic Principles of Chemistry:

A
  • Chemistry is the science of structure and interactions of matter
  • Matter is anything that has mass and takes up space
  • Mass is the amount of matter a substance contains, whereas weight is the force of gravity acting on a mass
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3
Q

Chemistry is the science of:

A

is the science of structure and interactions of matter

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4
Q

Matter is anything that has

A

anything that has mass and takes up space

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5
Q

Mass is the amount of

A

the amount of matter a substance contains, whereas weight is the force of gravity acting on a mass

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6
Q

Matter exists in 3 forms:

A
  • Solid
  • Liquid
  • Gas
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7
Q

4 elements that make up majority of our bodies:

A
  • nitrogen
  • oxygen
  • carbon
  • hydrogen
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8
Q

Oxygen symbol

A

O

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9
Q

Carbon symbol

A

C

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10
Q

Hydrogen symbol

A

H

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11
Q

Calcium symbol

A

Ca

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12
Q

Nitrogen symbol

A

N

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13
Q

Phosphorus

A

P

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14
Q

Potassium

A

K

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15
Q

Sodium

A

Na

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16
Q

Chlorine

A

Cl

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17
Q

Magnesium

A

Mg

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18
Q

Iron

A

Fe

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19
Q

Chemical elements are composed of:

A

Chemical elements are composed of units of matter of the same type called atoms

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20
Q

Atoms are the ___units of ___ that retain the ____ and ___of an element

A

Atoms are the smallest units of matter that retain the properties and characteristics of an element

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21
Q

Atomic number is the number of:

A

protons in nucleus of an atom

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22
Q

Mass number is the number of:

A

Mass number is the number of protons and neutrons in an atom

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23
Q

Neutron daltons =

A

Neutron = 1.008 daltons

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24
Q

Proton daltons=

A

Proton = 1.007 daltons

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25
Q

Electron daltons=

A

Electron = 0.0005 daltons

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26
Q

The atomic mass/weight of an element is:

A

The atomic mass/weight of an element is the average mass of all its naturally occurring isotopes

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27
Q

ion:

A

an atom that has lost or gained an electron

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28
Q

Cation aka

A

positive ion

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29
Q

anion aka

A

negative ion

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30
Q

Molecule

A

2 or more atoms sharing electrons

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31
Q

Compound:

A

Compound – a substance that can be broken down into 2 or more different elements

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32
Q

A chemical bond occurs when:

A

A chemical bond occurs when atoms are held together by forces of attraction

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33
Q

The number of electrons in the valence shell determines:

A

determines the likelihood that an atom will form a chemical bond with another atom

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34
Q

Hydrogen ion symbol and charge:

A

H+

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35
Q

Sodium ion symbol and charge:

A

Na+

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36
Q

potassium ion symbol and charge:

A

K+

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37
Q

Ammonium ion symbol and charge:

A

NH4 +

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38
Q

Magnesium ion symbol and charge:

A

Mg 2+

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39
Q

Calcium ion symbol and charge:

A

Ca2 +

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40
Q

Iron (II) ion symbol and charge:

A

Fe2 +

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41
Q

Iron (III) ion symbol and charge:

A

Fe3 +

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42
Q

Fluoride ion symbol and charge:

A

F-

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43
Q

Chloride ion symbol and charge:

A

Cl-

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44
Q

Iodide ion symbol and charge:

A

I-

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45
Q

Hydroxide ion symbol and charge:

A

OH-

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46
Q

Bicarbonate ion symbol and charge:

A

HCO3 -

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47
Q

Oxide ion symbol and charge:

A

O2-

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48
Q

Sulfate ion symbol and charge:

A

SO42-

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49
Q

Phosphate ion symbol and charge:

A

PO43-

50
Q

Ionic bond example:

A

NaCl

51
Q

Donated electron charge:

A

+ (excess of clothes for donation bin)

52
Q

Accepted electron charge:

A
  • (less clothes so accept more)
53
Q

Ionic bonding is through:

A

Ionic bonding is through the polarity of two atoms

54
Q

3 Type of covalent bonds:

A
  • Single
  • Double
  • Triple bonds
55
Q

Example of single covalent bond:

A

H2

56
Q

Example of double covalent bond:

A

O2

57
Q

Example of triple covalent bond:

A

N2

58
Q

Covalent bonds aka

A

Co dependent bond/couple; both offer something and are inseperable

59
Q

Hydrogen bonds result from:

A

Hydrogen bonds result from attraction of oppositely charged parts of molecules

60
Q

Hydrogen bonds between water molecules give water___:

A

Hydrogen bonds between water molecules give water cohesion

61
Q

Cohesion is the tendency of

A

Cohesion is the tendency of like particles to stay together

62
Q

Hydrogen bonds create:

A

Hydrogen bonds create surface tension

63
Q

Surface tension is a measure of

A

Surface tension is a measure of the difficulty of stretching or breaking the surface of a liquid

64
Q

Chemical reactions occur when:

A

Chemical reactions occur when new bonds are formed or old bonds are broken

65
Q

Reactants=

A

Reactants are starting substances

66
Q

Products=

A

Products are ending substances

67
Q

Metabolism is the sum of:

A

Metabolism is the sum of chemical reactions in the body

68
Q

Energy is the capacity to:

A

Energy is the capacity to do work

69
Q

Law of conservation of energy:

A

energy can neither be created nor destroyed but it can be converted from one form to another

70
Q

Potential energy aka

A

stored energy

71
Q

2 examples of potential energy:

A
  • Raising pen in air

- When rollercoaster rises to top

72
Q

2 examples of kinetic energy:

A
  • When pen is dropped

- When rollercoaster drops down

73
Q

Chemical energy:

A

-energy stored in bonds

74
Q

How do our bodies use chemical energy?:

A

We use it by breaking it apart

75
Q

Exergonic reactions is the releasing of:

A

Exergonic reactions is the releasing of energy

76
Q

Endergonic reactions bring ____ in:

A

Endergonic reactions bring energy in

77
Q

Example of exergonic reaction:

A

-Combustion

78
Q

Example of endergonic reactions:

A

-Melting ice; heat is brought in and causing melting

79
Q

Catalysts are used to lower:

A

-Catalysts are used to lower the activation energy in breaking it apart

80
Q

5 types of chemical reactions:

A
  • Synthesis
  • Decomposition
  • Exchange
  • Reversible
  • Oxidation-reduction
81
Q

An example of synthesis reaction:

A

-Synthesizing reactions together; hydrogen + oxygen = H2O

82
Q

An example of decomposition reaction:

A

Getting water and breaking it down into hydrogen and oxygen

83
Q

Example of exchange reaction:

A

When reactants change parts like ions, elements, or atoms

84
Q

Example of reversible reaction:

A

-reactants to products and can be reversed=

Sodium chloride+calcium carbonate=sodium carbonate+calcium chloride

85
Q

Oxidation reduction reactions:

A
  • reactions transfer electrons between atoms

- always occur in parallel (where when one substance is oxidized another is reduced)

86
Q

Oxidation=

A

loss of electrons and energy release

87
Q

Reduction+

A

gain of electrons and energy gain

88
Q

Inorganic compounds usually: (2)

A

Inorganic compounds

  • usually lack carbon
  • are simple molecules
89
Q

Water is the most ___and ____ inorganic compound in all living things

A

Water is the most important and abundant inorganic compound in all living things

90
Q

composition of Organic compounds: (3)

A
  • Organic compounds always contain H
  • always have covalent bonds
  • usually contain O
91
Q

Water is an ideal:

A

water is an ideal medium

92
Q

What type of molecule is water?

A

Water is a polar molecule

93
Q

Water solvent or solute?

A

Water is solvent

94
Q

In a hydrolysis reaction, water is:

A

In a hydrolysis reaction, water is added to break bonds

95
Q

In a dehydration synthesis reaction, water is:

A

In a dehydration synthesis reaction, water is removed to make bonds

96
Q

2 thermal properties of water:

A

Water has a:

  • High heat capacity
  • High heat of vaporization
97
Q

Water is a ___ ____ of our body fluids and helps ___ ____as membranes and organs slide over one another

A

Water is a major component of our body fluids and helps reduce friction as membranes and organs slide over one another

98
Q

Mixture:

A

a combination of elements or compounds that are physically blended together but not bonded together

99
Q

3 types of mixtures are:

A
  • solution
  • colloid
  • suspension
100
Q

Example of a solution:

A

-Salt water; light can pass through it

101
Q

Example of a colloid:

A

-homogenous and cloudy: milk

102
Q

Example of a suspension:

A

-Cloudy but can be separated: blood

103
Q

HCL; components and acid, base or salt?

A
  • H+ & Cl-

- acid

104
Q

KOH; components and acid, base or salt?

A
  • K+ & OH-

- base

105
Q

KCL; components and acid, base or salt?

A
  • K+ & Cl-

- salt

106
Q

(0)-6 PH =

A

Acidic

107
Q

7 PH =

A

Neutral

108
Q

8-(14) PH=

A

Basic

109
Q

Gastric Juice PH=

A

1.2-3.0

110
Q

Vaginal fluid PH=

A

3.5-4.5

111
Q

Urine PH=

A

4.6-8.0

112
Q

Saliva PH=

A

6.35-6.85

113
Q

Blood PH=

A

7.35-7.45

114
Q

Semen PH=

A

7.20-7.60

115
Q

Cerebrospinal fluid PH=

A

7.4

116
Q

Pancreatic Juice PH=

A

7.1-8.2

117
Q

Bile PH=

A

7.6-8.6

118
Q

Maintenance of body fluid homeostasis is…:

A

Maintenance of body fluid homeostasis is critical

119
Q

Buffer systems help to regulate pH by converting ____ or ___ into ____or _____

A

Buffer systems help to regulate pH by converting strong acids or bases into weak acids or bases

120
Q

4 facts about Carbons Compounds:

A
  • always contain carbon
  • combine in a variety of shapes
  • do not dissolve easily in water
  • good source of energy

currycurry UNIT ! (11 decks)

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