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Biological Foundations > Modules 1, 2 and 3 > Flashcards

Modules 1, 2 and 3 Flashcards

1
Q

Periodic Table

Which direction do the periods and groups go?

A

Periods - horizontal

Groups - verticle

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2
Q

Periodic Table

Do elements in periods or groups have similar chemical properties?

A

Groups (verticle)

e.g Noble gases, number of valence electrons are the same in a group

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3
Q

How is the periodic table arranged?

A

In increasing atomic number.

They are also grouped so elements with similar priperties are in the same column (group).

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4
Q

Nobel gasses?

A
  • Valence Shell is 8
  • Gas at room temperature
  • Happy not to form chemical bonds with other elements b/c valence shell is full
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5
Q

Non-metals?

A
  • Poor electriciy conductors
  • good heat conductors
  • cant bend and mould
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6
Q

Metals?

A
  • High electric and thermal conductors
  • can bend and be pulled out into thin wire
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7
Q

Representative Elements?

A

Elements in colums 1A to 7A

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8
Q

Transition elements?

A

Elements from 1B to 8B

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9
Q

Inner transition elements?

A

The ones pulled out and located at the bottom

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10
Q

Alkali metals?

A

Group 1A, not including Hydrogen (its a gas)

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11
Q

Alkaline metals?

A

Group 2A

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12
Q

Halogens?

A

Group 7A

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13
Q

Subatomic particles?

A
  • Protons,
  • Neturons
  • Electrons
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14
Q

Atomic number?

A

The number of protons

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15
Q

Mass number?

A

Protons + Neutrons

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16
Q

Isotope?

A

An element with a different number of neutrons to protons

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17
Q

Atomic mass?

A

The average mass number of all the isotopes of that element.

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18
Q

Chemical bond?

A

When 2 or more atoms are attracted to eachother either by sharing, or by losing and gaining electrons

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19
Q

Ionic bond?

A

The chemical bond formed when one atom or group gives up/transfers one or more electrons to another atom or group of atoms.

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20
Q

Covalent Bond

A

Where two or more atoms bond together by sharing electrons

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21
Q

Molecule

A

Two or more atoms bonded

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22
Q

Valence electrons

A
  • Electrons in outer shell
  • Elements in the same group have the same number of electrons in the outer valence shell
  • max # of valence electrons is 8
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23
Q

Lewis symbols

A
  • Number of calence velectons depicted by dots around the element symbol
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24
Q

Octet rule

A
  • Elements want to have 8 electons in its outer valence shell
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25
Q

Ions

A
  • Atoms that have either gained or lost one or more electrons
  • # protons and electrons are no longer the same
  • Electrically charged
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26
Q

Negatively charged Ion

A
  • An atom that has recieved electrons
  • More electrons than protons
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27
Q

Positively charged Ion

A
  • An atom that has lost electrons
  • More protons than electrons
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28
Q

Naming binary ionic compound rules

A

Full name of metal atom followed by first part of non-metal name + “ide”

  • MgO - Magnesium oxide
  • CaCL2 - Calcium chloride
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29
Q

Non-metal ions

A
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30
Q

Monatomic

A

One atom that has lost or gained electron/s

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31
Q

Polyatomic

A

Two ro more atoms bonded by losing and gaining electrons

  • HCO3 - hydrogen carbonate
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32
Q

Molecule

A

Two or more atoms bonded together

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33
Q

Cation

A

Positively charged ions

Add ‘ion’ to the end of the name

  • Ca2+ = Calcium ion

To help remember the ‘T’ in Cation is like a plus sign (+)

34
Q

Anion

A

Negatively charged ions

Add ‘ide’ to the end of the name

  • F- = Flouride
  • Cl-= Chloride

To help remember the ‘N’ in Anion represents negative (-)

35
Q

Polar molecule

A

Unequal sharing of electrons

36
Q

Non-polar molecule

A

equal sharing of molecules

37
Q

NO3-

A

Nitrate

38
Q

NH4+

A

Ammonium

39
Q

SO42-

A

Sulfate

40
Q

HSO4-

A

Hydrogen sulfate or bisulfate

41
Q

PO43-

A

Phosphate

42
Q

HPO42-

A

Hydrogen phoshate

43
Q

H2PO4-

A

Dihydrogen phosphate

44
Q

CO3-

A

Carbonate

45
Q

HCO3-

A

Hydrogen carbonate or bicarbonate

46
Q

CN-

A

Cyanide

47
Q

H3O+

A

Hydronium

48
Q

OH-

A

Hydroxide

49
Q

What are the main parts of a cell?

A
  1. Plasma membrane
  2. Cytoplasm - Organelles and cytosol
  3. Nucleus
50
Q

What is the smallest unit of matter that participates in chemical reactions?

A

Atom

51
Q

What is a molecule?

A

two or more atoms

52
Q

Which atoms (elements) are essential for maintaining life?

A
  • Carbon
  • oxygen
  • nitrogen
  • hydrogen
53
Q

What is chemistry?

A

The study of matter

54
Q

What is matter?

A

Anything that occupies space

55
Q
A
56
Q

What is a pure substance?

A
  • Elements
  • Compounds

Properties are always the same under the same conditions

57
Q

What is a mixture?

A
  • Physical combination of two or more substances
  • Properties and compositions can vary

eg

air is a mixture (homogenous)

soup is a mixture (heterogeneous)

58
Q

What is a homogenous mixture?

A

its is a mixture where the components cannot be seen

e.g. air

59
Q

What is a heterogenous mixture

A

a mixture where the you can see the components

e.g. vegetable soup

a glass of water with coins in it

60
Q

What is the difference between an element and a compond?

A

A compound can be broken down in to simpler substances, where as an elemant cant

61
Q

Chemical reactions

A
  • When new bonds of atoms form or existing bonds of atoms break down
  • It is the foundation of all life processes
  • the interaction of valence electrons

The number of atoms before and after a chemical reaction ate the same - just rearranged. The amount of energy at the beginning and end of the reaction is the same

62
Q

Reactants

A

The starting substances

  • 2H + O = H2O

The number of atoms before and after a chemical reaction ate the same - just rearranged. The amount of energy at the beginning and end of the reaction is the same

63
Q

Products

A

The ending substances

  • 2H + O = H2O

​The number of atoms before and after a chemical reaction ate the same - just rearranged. The amount of energy at the beginning and end of the reaction is the same

64
Q

Metabolism

A

All chemical reactions that occur in the body

65
Q

Energy

A

The capacity to do work

  1. Potential energy (stored by matter)
  2. kinetic energy (matter in motion)
66
Q

Chemical energy

A

A form of potential energy stored in the bonds of compounds and molecules

67
Q

Law of conservation of energy

A

Energy can be neither created or destroyed, it is converted to one form to another

68
Q

Activation energy

A

The collision energy need to break the chemical bonds of reactants.

Temperature and concentration of particles influence the change of collision

69
Q

Catalysts

A

Chemical compounds that

  • speed up chemical reactions
  • lower the need and amount of activation energy
  • dont change the amount of potential energy
  • assist with molecules hitting at the exact point needed for a reaction to occur

Catalysts remain unchanged and can assist in chemical reactions one after another

70
Q

Types of chemical reactions

A
  • Oxidation/reduction
  • Reversible
  • exchange
  • decomposition (catabolism)
  • Synthesis (anabolism)
71
Q

Anabolism

(synthesis reaction)

A
  • 2 or more atoms combining to form new and/or larger molecules
  • they absorb more energy than they release
72
Q

Catabolism

(decomposition reaction)

A
  • where larger molecules are split up into smaller molecules/atoms
  • uses more energy that they absorb
73
Q

Exchange reactions

A

Consists of both

  • Synthesis reaction (anabolism)
  • decomposition reaction (catabolism
74
Q

Reversible reactions

A
  • when products can revert back to their original reactants
  • many of these reactions in the body require catalysts (enzymes)
75
Q

Oxidation- Reduction reactions

A
  • AKA Redox reactions
  • when one substance os oxidised and another is equally reduced at the exact same time
  • loss and gain of electrons
76
Q

Oxidization

A

Loses electrons and released potential energy

77
Q

Reaction

A

Gains electrons and gains potential energy

78
Q

Displacement reactions

A

Movement of an atom from a compound to another atom to make a different compound

Fe + CuSO4 -> Cu + FeSO4

79
Q

Combustion reaction

A

Chemical reaction between a substance and oxygen (usually from air) that produces heat and light (usually from a flame)

most common type of chemical reaction

80
Q

Mole

A

6.02 x 1023 atoms in 12Carbon

A mole of any element contains 6.02 x 1023 atoms of that element

Molar mass (M) in grams = Relative atomic mass (RAM) in amu

81
Q

What are the three conditions required for a reaction to occur?

A
  1. Collision
  2. Orientation
  3. Energy
82
Q

What influences the chemical reaction rate?

A
  • Catalyst
  • Temperature - the hotter it is the easier for a collision to occur, molecules move faster
    • increase of 10 degrees doubles reaction rate
  • Concnetration - reaction rate increases when concentration of either or both reactants increases
  • The nature of the reactants -
    • reactions b/w ions in aqueous solution = very fast, activation energy low
    • reactions b/w covalent bonds (regardless in being in an aqueous solution) = slow, activtaion energy high

Biological Foundations (1 decks)

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