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Chemistry > Unit 1: Inorganic Chemistry > Flashcards

Unit 1: Inorganic Chemistry Flashcards

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1
Q

What is an element?

A

A pure substance consisting of only one type of atom

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2
Q

How many elements occur in nature?

A

92

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3
Q

4 elements that make up 96% of all living organisms?

A

Carbon
Oxygen
Hydrogen
Nitrogen

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4
Q

O

A

Oxygen
*cellular respiration, water

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5
Q

C

A

Carbon
*organic molecules

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6
Q

H

A

Hydrogen
*water, organic molecules, cellular respiration, pH

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7
Q

N

A

Nitrogen
*protein and nucleic acids

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8
Q

Ca

A

Calcium
*bones, teeth, muscle contraction, nerve impulses, blood clotting

major element

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9
Q

P

A

Phosphorous
*nucleic acids, bones

major element

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10
Q

K

A

Potassium
*major ion inside cells, nerve function

major element

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11
Q

S

A

Sulfur
*proteins

major element

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12
Q

Na

A

Sodium
*major cation in extracellular fluid, nerve function

major element

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13
Q

Cl

A

Chlorine
*major anion in extracellular fluid

major element

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14
Q

Mg

A

Magnesium
*enzyme component

major element

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15
Q

Si

A

Silicone

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16
Q

Al

A

Aluminum

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17
Q

Fe

A

Iron
*hemoglobin

trace element

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18
Q

Mn

A

Manganese
*fatty acid synthesis

trace element

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19
Q

F

A

Fluorine

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20
Q

V

A

Vanadium

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21
Q

Cr

A

Chromium
*glucose metabolism

trace element

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22
Q

Cu

A

Copper

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23
Q

B

A

Boron

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24
Q

Co

A

Cobalt

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25
Q

Zn

A

Zinc

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26
Q

Se

A

Selenium

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27
Q

Mo

A

Molybdenum

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28
Q

Sn

A

Tin

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29
Q

I

A

Iodine

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30
Q

What is an atom?

A

The smallest unit of an element

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31
Q

What is an atom made up of?

A

Protons
Neutrons
Electrons

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32
Q

What is the atomic nucleus?

A

Protons + neutrons

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33
Q

What determines the atomic weight?

A

The atomic nucleus (protons + neutrons)

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34
Q

What are the charges of the 3 subatomic particles?

A

Electrons: -
Protons: +
Neutrons: no charge

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35
Q

Where are electrons found in an atom?

A

Moving around the nucleus in the electron shell

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36
Q

What is the atomic number?

A

of protons in the nucleus

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37
Q

What is an ion?

A

A positively or negatively charged atom

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38
Q

What is an isotope?

A

Atoms that contain a different number of neutrons than normal

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39
Q

When are atoms most stable?

A

When their valence shells are complete with 8 electrons. (COHN incomplete, thus very chemically active)

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40
Q

What is the force behind the formation of bonds between atoms?

A

Activity of electrons

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41
Q

What is a molecule?

A

Two or more atoms of the same element (not a compound), or different elements (compound), that are chemically bonded

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42
Q

What is a compound?

A

A type of molecule made of atoms of different elements

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43
Q

What are the 3 types of mixtures?

A

Solutions
Colloids
Suspensions

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44
Q

What are solutions?

A

Homogeneous mixtures of various substances
Components can be liquid, solid, or gas
Usually clear

*Important because they help transfer gases between air, blood, and cells

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45
Q

What is a solvent?

A

Component of a solution with the greatest amount

46
Q

What is a solute?

A

Substance in a solution in smaller amount
Evenly distributed, do not settle

47
Q

What is a colloid (emulsion)?

A

Heterogeneous mixtures with larger solutes than solutions
Solutes reflect light, causing milky appearance
‘Sol-gel’ transformation: fluid -> solid -> fluid
eg. Jello

48
Q

What is a suspension?

A

Heterogeneous mixtures with very large solutes that separate when there is no movement
Can scatter light
Eg. Blood (will split into plasma and RBC)

49
Q

How do mixtures and compounds differ?

A
  1. Mixtures are physically mixed, not chemically bonded
  2. The components of mixtures can be separated, compounds can only be separated by breaking bonds
  3. All compounds are heterogeneous
50
Q

What is a chemical bond?

A

Atoms that share or transfer electrons as they try to fill their electron shell and become stable

51
Q

What is a covalent bond?

A

Strong bond where electrons are shared, spending part of their time in the shell of each atom

Single: 1 electron shared
Double: 2 electrons shared
Triple: 3 electrons shared

52
Q

What is a polar molecule?

A

A molecule with oppositely charged ends (results from shared electrons spending more time in one molecule than another)

(Electrons will spend more time near oxygen molecules in water)

53
Q

What is an ionic bond?

A

Electrons transferred from one atom to another
(Atoms with less than 2 electrons in their outer shell will likely ‘donate’, and those whose shell is almost full will ‘accept’)

54
Q

What is electrostatic attraction?

A

2 atoms drawn to each other by their electrical charges (ionic)

55
Q

What are ions?

A

Atoms with an electrical charge

56
Q

What is the difference between cations and anions?

A

Cations: positive charge
Anions: negative charge

57
Q

What is a hydrogen bond?

A

Not a true bond, electrons not shared/transferred
An electrostatic attraction between 2 hydrogen atoms due to different charges
Weak
Can form between molecules or between parts of same molecule

58
Q

What is a chemical reaction?

A

The formation and breaking of chemical bonds

59
Q

What is a chemical equation?

A

The written expression of a chemical reaction
X + Y -> Z
(X and Y: reactants, Z: product)

60
Q

What are the 3 types of chemical reactions?

A

Synthesis
Decomposition
Exchange

61
Q

What is a synthesis reaction?

A

Multiple smaller molecules/elements combine to form a new, complex chemical
Underlie all anabolic processes
- Requires energy

62
Q

What is a decomposition reaction?

A

A single chemical is broken down into multiple, smaller units
Foundation of catabolic reactions
- Releases energy

63
Q

What is an exchange reaction?

A

Atoms are exchanged between molecules (combo of synthesis + decomposition, bonds broken and made)
- No net energy requirement, the energy used from breaking bonds is used to create new ones

64
Q

What is activation energy?

A

The energy required for a reaction to happen

65
Q

What factors can influence the rate of reaction?

A

Concentration of reactants
Temperature

66
Q

What is a catalyst?

A

Special proteins (enzymes) that hold reactants together so they can interact
Not used up in the reaction
More catalysts = reaction speed increased

67
Q

What are organic compounds?

A

Complex molecules containing either C-C covalent bonds or C-H covalent bonds

68
Q

What are inorganic molecules?

A

Water, salt, acids, bases
Rarely have carbon, never hydrocarbon
Do not have C-C or C-H bonds
Tend to have ionic bonds

69
Q

What is a functional group?

A

Collections of atoms that attach to hydrocarbon chains, determine the functionality of the molecule
The reactive part of the molecule

70
Q

Why is carbon essential to organic molecules?

A

It has 4 valence shell electrons, and can thus form 4 covalent bonds. It can form long hydrocarbon chains that functional groups can then attach to.

71
Q

What are some important roles of water?

A
  • Universal solvent: layer of water forms around each molecule
  • Ideal transport medium: carries nutrients, waste, hormones, gases. etc.
  • Temperature moderation: absorbs heat from reactions
  • Lubricant
  • Protection: cushioning effect
72
Q

What is salt?

A

Mineral compound with ionic bonds, principal form of minerals in the body
Dissociate in water and release ions
When solid, contain both cation and anions (cancel out - no net charge)
Important for nerve impulses and muscle contractions

73
Q

What is an electrolyte?

A

Ionic form of salt (when salt is added to water it ionizes [divides into separate ions])

74
Q

What is an acid?

A

Ionically bonded substance that releases hydrogen ions when added to water (AKA they ‘ionize’)
Called ‘proton donors’ (H+ is a proton, no electrons)
Electrolyte
*acids lower the pH

75
Q

What is a base?

A

Alkaline compound ionically bonded
Ionize in water to release hydroxyl ions (OH-)
Known as ‘proton acceptors’
OH- attracted to H+ from acids -> form water
Electrolyte
*bases raise the pH

76
Q

What pH is healthy in animal tissues and blood?

A

7.4

77
Q

What is a buffer?

A

A solution with the ability to resist changes in pH
Weak acids and bases that do not completely ionize in water
Keeps the pH in the neutral range by either picking up or releasing H+ ions

78
Q

What is the most common buffer system?

A

Carbonic acid (H2CO3) + bicarbonate (HCO3-)

79
Q

What pH level is basic/alkaline?

A

> 7 - 14

80
Q

What pH level is acidic?

A

<7 - 0

81
Q

What makes bicarbonate an effective buffer?

A

Its ability to act as both a weak acid (loses a proton) and a weak base (gains a proton)

82
Q

NaCl

A

Sodium chloride (table salt)

83
Q

What are the 4 major cations of animals?

A

Na, K, Ca, Mg

84
Q

What are 3 major anions of animals?

A

Cl, HCO3 (bicarbonate), PO4 (phosphate)

85
Q

What are 4 ways to increase the formation of a solution?

A
  1. Grinding the solute
  2. Heating
  3. Stirring
  4. Shaking
86
Q

What is intravascular fluid?

A

Water in lymphatic and blood vessels

87
Q

What is interstitial fluid?

A

Water outside vessels and surrounding cells

88
Q

What percent of body water is intracellular?

A

2/3

89
Q

What percent of water is extracellular?

A

1/3

90
Q

What are properties of salt in an aqueous solution?

A

Conduct electricity
Boil at higher temperatures
Freeze at lower temperatures

91
Q

What are strong electrolytes?

A

Ions dissociate completely
Highly soluble
Solutions of strong electrolytes readily conduct electric currents

92
Q

What are weak electrolytes?

A

Ions dissociate slightly
Poorly soluble.
Collect electric currents poorly

93
Q

Most body fluids are solutions of…?

A

Electrolytes

94
Q

What is blood a mixture of?

A

Cells + proteins suspended in plasma (liquid)

95
Q

What do acids and bases form when they come together?

A

H+ (acid) + OH- (base) = H2O
Water (helps to neutralize a solution)

96
Q

What pH should blood plasma be?

A

7.35 - 7.45

97
Q

What are 3 methods of buffering the body uses to maintain normal H+ levels?

A
  1. Combining H+ with either a blood or intracellular buffer
  2. Reduction of carbonic acid through elimination of CO2 from lungs
  3. Renal elimination of H+
98
Q

Concentrations of ___ determine blood pH?

A

Bicarbonate and carbonic acid
(Normally 1 part carbonic to 20 parts bicarbonate)

99
Q

What is acidosis?

A

pH of arterial blood below 7.35
- Respiratory acidosis: too much CO2 -> pH decreases, need more H (eg. hyperventilation)
- Metabolic acidosis: blood H+ levels increase -> pH decrease, need more CO2 (eg. kidney failure)

100
Q

What is alkalosis?

A

pH of arterial blood above 7.45
- Respiratory alkalosis: loss of CO2, pH increases
- Metabolic alkalosis: loss of H+, pH increases

101
Q

How can the body compensate for alkalosis and acidosis?

A

Alkalosis: decrease respiratory rate
Acidosis: increase respiratory rate

Long term compensation done through kidneys

102
Q

What are the 4 major cations found in animals?

A

Na+ (sodium)
K+ (potassium)
Ca+ (calcium)
Mg+ (magnesium)

103
Q

What are the 3 major anions found in animals?

A

Cl- (chloride)
HCO3- (bicarbonate).
PO4- (phosphate)

104
Q

What is the solvent of an aqueous solution?

A

Water

105
Q

What dissolves well in aqueous solutions?

A

Salts (split into ions in water)
Some organic molecules (not ionized)

106
Q

Why are solutions biologically useful?

A

Exert osmotic pressure
Contain ions
Can buffer

107
Q

What are the 4 types of inorganic molecules important for life?

A

Water
Salts
Acids
Bases

108
Q

Water solubility of 3 important ions?

A

Calcium Chloride (CaCl2): 745
Sodium Chloride (NaCl): 361
Calcium Phosphate (Ca3(PO4)2): 0.002

109
Q

What are the major ions in plasma and interstitial fluid?

A

Na+ and Cl-

110
Q

What are the major ions in intracellular fluid?

A

K+ and HPO4-

111
Q

What does the pH scale measure?

A

H+ ion concentration

112
Q

How do buffers work?

A

Buffer = solution that resists pH changes
Do NOT completely ionize in water
Balance H+, either by picking up or releasing H+

Chemistry (5 decks)

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