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A&P Lecture Unit 1 > Chapter 2 A&P Lecture > Flashcards

Chapter 2 A&P Lecture Flashcards

Basic and Inorganic Chemistry

1
Q

Anything that has mass and occupies space?

A

Matter

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2
Q

Pull of gravity on mass?

A

Weight

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3
Q

What are the 3 states of matter?

A

Solid, Liquid, Gas

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4
Q

Which state of matter has a definite shape and volume?

A

Solid

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5
Q

Which state of matter has a changeable shape; definite volume?

A

Liquid

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6
Q

Which state of matter has a changeable shape and volume?

A

Gas

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7
Q

Capacity to do work or put matter into motion?

A

Energy

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8
Q

What are the types of energy and their definitions?

A

Kinetic- energy in action

Potential- stored (inactive) energy

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9
Q

Can energy be transferred from potential to kinetic energy?

A

Yes

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10
Q

What are the forms of energy?

A

Chemical energy
Electrical energy
Mechanical energy
Radiant or electromagnetic energy

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11
Q

What form or energy is stored in bonds of chemical substances?

A

Chemical energy

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12
Q

What form or energy results from movement or charged particles?

A

Electrical energy

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13
Q

What form or energy is directly involved in moving matter?

A

Mechanical energy

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14
Q

What form or energy travels in waves (e.g. visible light, ultraviolet light, and x-rays)?

A

Radiant or electromagnetic energy

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15
Q

Can energy be converted from one form to another?

A

Yes

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16
Q

Is energy conversion efficient?

A

No, because some energy is “lost” as heat (partly unusable energy)

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17
Q

Matter is composed of?

A

Elements

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18
Q

True or False: Elements cannot be broken into simpler substances by ordinary chemical methods.

A

True; elements CANNOT be broken into simpler substances by ordinary chemical methods.

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19
Q

What are the unique properties of an element?

A

Physical properties and Chemical Properties

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20
Q

Define physical properties

A

Physical properties are detectable with our senses or are measurable.

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21
Q

Define Chemical properties

A

Chemical properties are how atoms interact (bond) with one another.

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22
Q

What are the unique building blocks for each element?

A

Atoms

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23
Q

What gives each element its physical and chemical properties?

A

Atoms

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24
Q

True or False: Atoms are the smallest particles of an element with properties of that element.

A

True: Atoms are the smallest particles of an element with properties of that element.

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25
Q

What is an atomic symbol?

A

One or Two letter chemical shorthand for each element often the first letter of the element’s name.

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26
Q

What are the 4 elements that make up 96.1% of body mass?

A

Carbon -C
Hydrogen -H
Oxygen -O
Nitrogen -N

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27
Q

What re the 9 elements that make of 3.9% of body mass?

A 
Element:       Atomic Symbol:
Calcium                 Ca
Phosphorus           P
Potassium              K
Sulfur                     S
Sodium                  Na 
Chlorine                 Cl
Magnesium             Mg
Iodine                      I
Iron                         Fe
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28
Q

What are the trace elements (found in very minute amounts) found in the body?

A 
Chromium    Cr
Copper    Cu
Fluorine    F
Manganese    Mn
Silicon    Si
Zinc    Zn
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29
Q

What are atoms composed of?

A

Subatomic particles: Protons, Neutrons, Electrons

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30
Q

What subatomic particles are found in the nucleus?

A

Protons and neutrons

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31
Q

Which subatomic particle orbits the nucleus in the electron cloud?

A

Electrons

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32
Q

What makes of almost the entire mass of the atom?

A

The nucleus

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33
Q

Do neutrons or protons carry a charge?

A

Protons, which have a positive charge. Neutrons carry no charge.

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34
Q

What is the mass of a neutron?

A

Neutron mass = 1 atomic mass unit (amu)

Proton mass = 1 amu

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35
Q

What charge does an electron have when in orbitals within electron cloud?

A

Electrons carry a negative charge

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36
Q

What is the mass of an electron when in orbitals within electron cloud?

A

1/2000 (0 amu)

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37
Q

Are the number of protons usually equal to electrons?

A

Yes, they are equal in an atom of an element.

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38
Q

Which model of an atom is depicted with probable regions of greatest electron density (an electron cloud) and is useful for predicting chemical behavior of atoms?

A

The Orbital Model - current model used by chemists

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39
Q

Which model of an atom incorrectly depicts a simplified and fixed circular electron paths?

A

Planetary model -used for illustrative purposes in textbooks only and is outdated with the onset of the Orbital model.

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40
Q

What determines what an element IS?

A

The number of protons, the atomic number of an element. 47 protons will Always be Silver.

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41
Q

How is a mass number determined?

A

By adding the total number of Protons + Neutrons in the nucleus. This is the total mass of an atom.

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42
Q

How is the mass number depicted?

A

Written as superscript to left of atomic symbol

Ex. 7th power Li

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43
Q

The number of protons in the nucleus is the …?

A

Atomic number

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44
Q

How is the atomic number depicted?

A

Written as subscript to left of atomic symbol

Ex. tiny 3 below the line Li

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45
Q

What is a structural variation of atoms?

A

Isotopes

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46
Q

How do isotopes differ from their original element?

A

They differ in the number of neutrons they contain, and their atomic numbers remain the same while their mass number is different

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47
Q

What are heavy isotopes that decompose to more stable forms and can be detected with scanners?

A

Radioisotopes

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48
Q

What is the term for spontaneous decay?

A

Radioactivity

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49
Q

What is the atomic symbol for Carbon?

A

C

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50
Q

What is the atomic symbol for Hydrogen?

A

H

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51
Q

What is the atomic symbol for Oxygen?

A

O

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52
Q

What is the atomic symbol for Nitrogen?

A

N

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53
Q

What is the atomic symbol for Phosphorous?

A

P

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54
Q

What is the atomic symbol for Sulfur?

A

S

55
Q

What is the atomic symbol for Calcium?

A

Ca

56
Q

What is the atomic symbol for Iron?

A

Fe

57
Q

What is the atomic symbol for Sodium?

A

Na

58
Q

What is the atomic symbol for Potassium?

A

K

59
Q

What is the atomic symbol for Chlorine?

A

Cl

60
Q

What is the atomic symbol for Magnesium?

A

Mg

61
Q

What is the atomic symbol for Chromium?

A

Cr

62
Q

What is the atomic symbol for Iodine?

A

I

63
Q

What is the atomic symbol for Cobalt?

A

Co

64
Q

What is the atomic symbol for Fluorine?

A

F

65
Q

What is the atomic symbol for Vanadium?

A

V

66
Q

What is the atomic symbol for Selenium?

A

Se

67
Q

What is the atomic symbol for Manganese?

A

Mn

68
Q

What is the atomic symbol for Copper?

A

Cu

69
Q

What is the atomic symbol for Zinc?

A

Zn

70
Q

What is the atomic symbol for Silicon?

A

Si

71
Q

What is the atomic symbol for TIn?

A

Sn

72
Q

What is the atomic symbol for Molybdenum?

A

Mo

73
Q

A stable atom has the same number of…?

A

Protons and electrons

74
Q

of protons determines an element’s…?

A

Atomic Number

75
Q

An atom that has either gained or lost electrons is called?

A

An ion

76
Q

An atom that has gained electrons is called?

A

A negative ion/Anion

77
Q

An atom that has lost electrons is called?

A

A positive ion/cation

78
Q

2 or more of the same kind of atoms joined by chemical bonds?

A

Molecules

79
Q

2 or more of different types of atoms proportions designated by a chemical formula is called

A

A compound

80
Q

An atom that has gained electrons is called?

A

The electron acceptor which is now a negative ion/Anion

81
Q

An atom that has lost electrons is called?

A

The electron donor which is now called a positive ion/cation

82
Q

What makes the nucleus positively charged overall?

A

Because protons are positively charged and neutrons have not charge.

83
Q

The number of protons is always equal to the # of electrons in an atom, so the atomic # indirectly tells us the # of _____ in the atom as well.

A

Electrons

84
Q

To figure out the number of protons, look at the ?

A

Bottom subscript, the atomic number. The atomic number is the number of protons.

85
Q

To figure out the number of electrons, look at the

A

Bottom subscript, the atomic number since in a neutral atom, the number of protons and electrons are the same number.

86
Q

How to figure out the number of neutrons?

A

Subtract the top number (mass number) from the bottom number (atomic number) to find the number of neutrons.

87
Q

What are elements that have the same number of protons (and electrons), but differ in the # of neutrons they contain?

A

Isotopes

88
Q

Elements shown on the periodic table usually represent

A

The most abundant types/forms of an element.

89
Q

What subatomic particle does not change in isotopes?

A

The number of protons the element has, otherwise, Carbon would not be Carbon, for example.

90
Q

What is another way that isotopes can be written?

A

Carbon : C-14 to represent the mass number instead of the top subscript.

91
Q

How many neutrons does the carbon isotope C-12, C-13, and C-14 have, respectively when Carbon has 6 protons?

A

C-12 has 6 neutrons,
C-13 has 7 neutrons,
C-14 has 8 neutrons

Subtract the atomic mass from the atomic number to find the number of neutrons.

92
Q

What is the definition of a “molecule of an element”

A

A molecule that has more than one of the same element such as 2 Oxygen atoms comboned, shown as O2 or 8 Sulpfur atoms: S8 (the number is a bottom subscript).

93
Q

When two more more DIFFERENT kinds of atoms bind…

A

…they form a compound such as H2O or CH2

94
Q

Just as an atom is the smallest particle of an element, a molecule is the smallest particle of a

A

Compound. Compounds are therefore chemically pure.

95
Q

What is the definition of a “molecule of an element”

A

A molecule that has more than one of the same element such as 2 Oxygen atoms combined, shown as O2 or 8 Sulfur atoms: S8 (the number is a bottom subscript).

96
Q

3 types of mixtures are

A

Solutions, Colloids, Suspensions

97
Q

When two or more DIFFERENT kinds of atoms bind…

A

…they form a compound such as H2O or CH2

98
Q

Define hetergenous mixture

A

A mixture that contains dissimilarities in different areas of the mixture. Randomly selected areas would differ from other areas of the mixture.

99
Q

The substance found in the greatest amount within a mixture is called?

A

The solvent.

100
Q

The substance in smaller amounts of the mixture/

A

The solute.

101
Q

In the body, most Solutions are ___?

A

True solutions containing gases, liquids and solids dissolved in water. Usually transparent that do not scatter light e,g. atmospheric air or saline solution.

102
Q

If glucose is dissolved in blood, the glucose would be the ____ and the blood would be the ____.

A

Solute

Solvent

103
Q

Concentration of true solutions can be expressed as:

A

Percent of solute in total solution (assumed to be water)
Milligrams per deciliter (mg/dl)
Molarity, or moles per liter (M)

104
Q

Percent of solute in total solution (assumed to be water)?

A

Parts solute per 100 parts solvent

105
Q

Molarity, or moles per liter (M)?

A

1 mole of an element or compound = Its atomic or molecular wight (sum of atomic weights ) in grams

1 mole of any substance contains 6.02 x 10 to the 23rd power molecules of that substance (Avogadro’s number).

106
Q

A mixture that is hetergenous with large solute particles that do NOT settle out

A

Colloids a,k,a Emulsions.

Some undergo sol-gel transformations e.g. cytosol during cell divison.

107
Q

A mixture that is heterogenous and has large visible solutes that settle out.

A

Suspensions such as blood

108
Q

Mixture or Compound? No chemical bonding between components.

A

Mixture

109
Q

Mixture or Compound? Chemical bonding between components.

A

Compound

110
Q

Mixture or Compound? Can be separated by physical means such as straining or filtering

A

Mixture

111
Q

Mixture or Compound? Can be separated only by breaking bonds

A

Compounds

112
Q

Mixture or Compound? can be either Hetergenous or homogenous.

A

Mixture

113
Q

Mixture or Compound? All all homogenous

A

Compound

114
Q

Nuclear attraction is strongest between the positively charged nucleus and the negatively charged electrons.. where/

A

The closer the electrons are located to the nucleus, the stronger the pull toward it. The further it is away from the nucleus, the more likely it is to chemically interact with other atoms.

115
Q

Define the rule of eights.

A

The outermost shell, called the valance shell, is not stable until it has 8 electrons.

116
Q

What makes an atom chemically inert?

A

If the valence shell has 8 electrons. Noble gasses such as helium and neon are inert.

117
Q

Most ionic compounds are ____?

A

Salts. When dry salts form crystals instead of indie molecules. Example: NaCl (Sodium Chloride).

118
Q

What happens to the two ions after electron transfer?

A

They become attracted to each other since they are now oppositely charged, and combine to form an ionic bond such as Sodium chloride.

119
Q

What happens to the two ions after electron transfer?

A

They become attracted to each other since they are now oppositely charged, and attract to form an ionic bond such as Sodium chloride.

120
Q

A bond formed when two or more electrons are shared between atoms to achieve stability.

A

Covalent bond.

121
Q

The type of covalent bond where electrons are shared equally, and produces electrically balanced, nonpolar molecules such as CO2

A

Nonpolar covalent bonds. They always appear linear and symmetrical

122
Q

The type of covalent bond that is the unequal sharing of electrons which produces polar (aka dipole) molecules such as H2O

A

Polar covalent bonds. The molecules always look v-shaped bc it has 2 poles of charge - a slightly more negative oxygen end and a slightly more positive hydrogen end.

123
Q

Small atoms with 6 or 7 valances shell electrons which create a strong electron attracting ability are _______?

A

Electronegative e.g. oxygen

124
Q

Most atoms with 1 or 2 valance shell electons which create a weaker ability to attract and often cause them to lose electrons are _______

A

Electropositive e.g. sodium

125
Q

The type of covalent bond where electrons are shared equally, and produces electrically balanced, nonpolar molecules such as CO2, and always appear linear and symmetrical.

A

Nonpolar covalent bonds.

126
Q

Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule

A

Hydrogen bond

127
Q

Bond which does not offer a true bond but acts mostly as intramolecular bonds, holding a large molecule in a 3D shape. Commonly between dipoles such as water.

A

Hydrogen bond

128
Q

A chemical reaction that is constructive is called

A

Anabolic

129
Q

A chemical reaction that is destructive is called

A

Catabolic

130
Q

What happens in an exergonic reaction?

A

Energy is liberated

131
Q

What happens in an endergonic reaction?

A

Energy is absorbed

132
Q

If reaction conditions remain unchanged, all chemical reactions eventually reach a state of

A

Chemical equilibrium

133
Q

What are some things that increase reaction rate?

A

Higher temp
Presence of catalysts
The smaller the reacting particles are

134
Q

What is the single most abundant compound in the body which absorbs and releases heat slowly, acts as a universal solvent, participates in chemical reactions, and cushions body organs?

A

Water

A&P Lecture Unit 1 (6 decks)

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