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BMS 191 > 2. Chemistry > Flashcards

2. Chemistry Flashcards

1
Q

Matter

A

Anything that takes up space and has mass

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2
Q

Two purity bases of matter

A
  1. Pure substance

2. Mixture

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3
Q

Pure substance

A

Only made of one type of material. e.g helium gas (only He)

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4
Q

Mixture

A

Made up of 2 or more different substances, can be operated by physical means. e.g H20 (hydrogen and oxygen)

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5
Q

Classification of matter

A

Atom

Element

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6
Q

Atom

A

Smallest unit of matter, cannot be cut, inseparable

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7
Q

Element

A

A substance made up of one type of atom and the properties of that substance

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8
Q

States of matter

A

Solids
Liquids
Gases

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9
Q

Solids

A

Definite shape and occupy definite volume

Strong forces of attraction, atoms don’t move much

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10
Q

Liquids

A

No definite shape, occupy definite volume
Lower force of attraction, molecules have more energy
Molecules slide across each other

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11
Q

Gases

A

No definite shape, no definite volume

Molecules had so much energy, they move too fast, breaking the forces of attraction

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12
Q

Two factors that influence states of matter

A
  1. Forces of attraction between molecules (strong/weak)

2. Molecules vibrate

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13
Q

Two categories for pure substances

A
  1. Element

2. Compound

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14
Q

Element

A

Atoms are the same (O2), (H2)

Cannot be broken down into two or more different substances. e.g oxygen

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15
Q

Compound

A

Atoms are different (CO2), (H2O)
A substance made up of two or more atoms which are from different elements.
Can be broken down into the elements contained in them

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16
Q

Two categories for Mixtures

A
  1. Homogenous mixture

2. Heterogenous mixture

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17
Q

Molecule

A

A substance made up of two or more atoms from either an element of compound.

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18
Q

Structure of an atom

A

Nucleus
Protons
Nuetrons
Electrons

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19
Q

Nucleus

A

Made up of a number of particles that are smaller than the atom

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20
Q

Protons

A

Positively charged particles in the nucleus

Number of protons determines what element the atom is

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21
Q

Neutrons

A

No charge
Subatomic particle in the nucleus
Help keep the nucleus together

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22
Q

Electrons

A

Negatively charged

Number of electrons is always equal to the number of protons

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23
Q

Atomic number

A

Number of protons that are present in an atom (top left corner) or top middle

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24
Q

Mass number

A

Number of protons + number of neutrons

Always a whole number

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25
Q

Atomic mass

A

Average of the number of protons and neutrons

Decimal number

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26
Q

Isotopes

A

An element that has the same number of protons but different number of neutrons

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27
Q

Electrons shells

A

Where the electrons are found

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28
Q

How many electrons in the first shell?

A

2

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29
Q

How many electrons in the second and third shell?

A

8

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30
Q

Valence shell

A

The outermost electron shell

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31
Q

Octet rule

A

The tendency to have 8 electrons in their second and third electron shell

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32
Q

Types of chemical bonds (4)

A
  1. Ionic bonds
  2. Covalent bonds
  3. Metallic bonds
  4. Hydrogen bonds
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33
Q

Ionic bonds

A

There is a physical exchange of an electron from the valence shell of one atom to the valence shell of another atom

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34
Q

Ion

A

When an atom has an unbalanced charge

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35
Q

Cations (t for +)

A

Ions that have a net positive charge (more protons than electrons)

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36
Q

Anions

A

Ions that have net negative charge (more electrons then protons)

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37
Q

Covalent bonds

A

Atoms achieve full valence shells by sharing electrons

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38
Q

Non-polar covalent bonds

A

Sharing of electrons is equal, so the resulting molecule has no charge associated with it. E.g carbon dioxide

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39
Q

Polar-covalent bonds

A

Sharing of electrons is uneven (electrons spend more time near one atom than the other)

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40
Q

Metallic bonds

A

Sharing of free electrons among a structure of positively charged ions

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41
Q

Hydrogen bonds

A

Weaker interactions that alter the way molecules interact with each other

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42
Q

Chemical reactions

A

The process which new bonds between atoms are formed, or where existing bonds between atoms are broken

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43
Q

Two components of chemical reactions

A
  1. Reactants - molecules present at the start

2. Products -molecules present at the end

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44
Q

Energy

A

The capacity for doing work/causing change

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45
Q

Two main forms of energy

A
  1. Potential energy

2. Kinetic energy

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46
Q

Potential energy

A

Energy store by matter due to its position

Chemical, electrical, nuclear

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47
Q

Kinetic energy

A

The energy associated with matter in motion

mechanical, thermal

48
Q

Exothermic reaction (exergonic)

A

Chemical reactions that result in the release of energy

ex for exit

49
Q

Endothermic reaction (endergonic)

A

reactions absorb energy in the form of heat. e.g ice pack on wrist

50
Q

Types of reactions

A 
REDS
R - reversible
E - exchange
D - decomposition
S - synthesis
51
Q

Reversible reaction

A

Reaction can proceed in both directions

52
Q

Exchange reaction

A

When one atom/functional group replaced another in a compound

53
Q

Decomposition

A

A larger molecule is broken apart into simpler substances

54
Q

Synthesis

A

two or more atoms/molecules are bonded together to form a more complex molecule

55
Q

Metabolism

A

The chemical processes that occur within the cells of a living organism to maintain life

  • Breakdown and assembly of molecules
  • Reaction energy output or input
56
Q

Catabolism

A

Breakdown of molecules

57
Q

Anabolism

A

Building of molecules

58
Q

Activation energy

A

The energy required to initiate a chemical reaction

59
Q

Catalyst

A

A chemical substance that acts to lower the activation energy required for certain chemical reactions

60
Q

Enzymes

A

Proteins that act as a catalyst

61
Q

Mixtures

A

A combination of elements or compounds that are physically blended together

62
Q

Solvent

A

A liquid or gas that is able to dissolve other substances

63
Q

Solute

A

A substance that is dissolved into solvent

64
Q

Solution

A

A mixture of a solute dissolved into a solvent, remains evenly distributed

65
Q

Colloid

A

A mixture of a solute and solvent, but where the solute particles are large enough to scatter light as it passes through

66
Q

Suspension

A

A mixture of particles in a liquid for a period of time, but eventually it will settle out of the liquid

67
Q

Concentration

A

The proportion of solute dissolved in a solvent (high/low)

68
Q

High concentration

A

High amount of solute

69
Q

Low concentration

A

Low amount of solute

70
Q

Terms to describe the concentration of a solute (3)

A

Mass
Percentage
Molarity: number of molecules present

71
Q

Mole

A

Unit of measurement for amount of substance

72
Q

Molecular weight/mass

A

Sum of the atomic weight/mass of all elements contained within the molecular that makes a compound

73
Q

Molarity of a solution

A

Number of moles of solute dissolved in 1L of solvent

74
Q

Acids

A

A substance that separates when dissolved in water and releases hydrogen ions

75
Q

Bases (alkali)

A

A substance that separates when dissolved in water and releases hydrogen ions

76
Q

Salts

A

Any compound that results from the chemical interaction of an acid and a base

77
Q

Strong/weak acids

A

Strong acid - a substance that has a strong tendency to separate completely and release hydrogen ions

Weak acid - a substance that has a weak tendency to separate and release hydrogen ions

78
Q

Strong/weak bases

A

Strong base - a substance that has a strong tendency to separate completely and release hydroxide ions

Weak bases - a substance that has a weak tendency separate to release hydroxide ions

79
Q

pH (potential hydrogen)

A

Measure of the concentration of hydrogen ions in a solution

80
Q

pH levels below 7 (<7) =

A

Acidic

81
Q

pH levels of 7 =

A

Neutral

82
Q

pH levels above 7 (>7) =

A

Basic (alkaline)

83
Q

Buffer

A

A substance that is able to remove or ad hydrogen ions and is able to resist large changes in pH

84
Q

Organic molecules

A

Those that contain the element carbon

85
Q

Four types of organic molecules

A
  1. Carbohydrates
  2. Lipids
  3. Proteins
  4. Nucleic acids and nucleotides
86
Q

What compounds are carbohydrates?

A

Sugars
Glycogen
Starches
Cellulose

87
Q

Function of carbohydrates

A

Source of chemical energy

The energy released when carbohydrates are broke down are the molecules of ATP

88
Q

Three major groups of carbohydrates based on size

A
  1. Monosaccharides
  2. Disaccharides
  3. Polysaccharides
89
Q

Monosaccharides

A

one saccharide molecule

mono = 1

90
Q

Disaccharides

A

Molecules that are formed by the joining together of two monosaccarides
di = 2

91
Q

Polysaccharides

A

Molecules that are formed by the joining together of tens or hundreds of monosaccharides
poly= many

92
Q

Main polysaccharide in the body

A

Glycogen

93
Q

Main polysaccharides produced by plants

A

Starches and Cellulose

94
Q

Main types of lipids in the body

A

Fatty acids
Phospholipids
Steroids

95
Q

Function of proteins

A

Form enzymes which catalyse chemical reactions in the body

Form antibodies to detect invading microbes

96
Q

Dipeptide

A

Two amino acids joined together

di = 2

97
Q

Tripeptide

A

Three amino acids joined together

tri = 3

98
Q

Polypeptide

A

Tens of thousands of amino acids joined together

poly= many

99
Q

Amino acids

A

Building blocks for proteins

100
Q

Four levels of structural organisation of proteins

A
  1. Primary
    2, Secondary
  2. Tertiary
  3. Quaternary
101
Q

Primary structure of a protein

A

Sequence of amino acids linked together by peptide bonds to form a polypeptide

102
Q

Secondary structure of a protein

A

The repeated twists and folding that the polypeptide chain undergoes

103
Q

Tertiary structure of a protein

A

Three dimensional folding pattern of a protein due to side chain interactions

104
Q

Quaternary structure of a protein

A

The combination of different polypeptides to form a single functional protein

105
Q

Denaturation

A

The breaking down of a protein three dimensional shape

106
Q

Two forms of nucleic acid in the body

A
  1. Deoxyribonucleic acid (DNA)

2. Ribonucleic acid (RNA)

107
Q

Three components of a nucleotide

A
  1. A nitrogenous base
  2. A sugar composed of 5 carbons
  3. A phosphate group
108
Q

4 nitrogenous bases (nucleotides)

A

Thymine (T) - Adenine (A)
(the apple (A) falls of the tree (T))

Cytosine (C) - Guanine (G)

109
Q

What is replaced in RNA

A

Uricil (U) replaces Thymine (T)

110
Q

Function of ATP

A

Acts as a storage molecule for energy

111
Q

Radiation

A

The travel of energy either as particles or as electromagnetic waves

112
Q

Types of radiation

A

Ionising radiation

Non- ionising radiation

113
Q

Ionising radiation

A

Has enough energy to strip electrons away from other atoms. e.g x-rays, alpha, beta, gamma rays

114
Q

Non-ionising radiation

A

Can interact with materials but it does not have enough energy to move electrons. e.g microwaves

115
Q

Nuclear radiation

A

The release of radiation due to the breakdown of an atoms nucleus

116
Q

Types of radiation nuclear decay can produce

A
  1. Alpha rays
  2. Betta rays
  3. Gamma rays
117
Q

Two types of radiation damage

A

Direct

Indirect

BMS 191 (3 decks)

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