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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
Ions
* Atoms that have either gained or lost one or more electrons * # protons and electrons are no longer the same * Electrically charged
26
Negatively charged Ion
* An atom that has recieved electrons * More electrons than protons
27
Positively charged Ion
* An atom that has lost electrons * More protons than electrons
28
Naming binary ionic compound rules
Full name of metal atom followed by first part of non-metal name + "ide" * MgO - Magnesium oxide * CaCL2 - Calcium chloride
29
Non-metal ions
30
Monatomic
One atom that has lost or gained electron/s
31
Polyatomic
Two ro more atoms bonded by losing and gaining electrons * HCO3 - hydrogen carbonate
32
Molecule
Two or more atoms bonded together
33
Cation
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
Anion
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
Polar molecule
Unequal sharing of electrons
36
Non-polar molecule
equal sharing of molecules
37
NO3-
Nitrate
38
NH4+
Ammonium
39
SO42-
Sulfate
40
HSO4-
Hydrogen sulfate or bisulfate
41
PO43-
Phosphate
42
HPO42-
Hydrogen phoshate
43
H2PO4-
Dihydrogen phosphate
44
CO3-
Carbonate
45
HCO3-
Hydrogen carbonate or bicarbonate
46
CN-
Cyanide
47
H3O+
Hydronium
48
OH-
Hydroxide
49
What are the main parts of a cell?
1. Plasma membrane 2. Cytoplasm - Organelles and cytosol 3. Nucleus
50
What is the smallest unit of matter that participates in chemical reactions?
Atom
51
What is a molecule?
two or more atoms
52
Which atoms (elements) are essential for maintaining life?
* Carbon * oxygen * nitrogen * hydrogen
53
What is chemistry?
The study of matter
54
What is matter?
Anything that occupies space
55
56
What is a pure substance?
* Elements * Compounds Properties are always the same under the same conditions
57
What is a mixture?
* Physical combination of two or more substances * Properties and compositions can vary eg air is a mixture (homogenous) soup is a mixture (heterogeneous)
58
What is a homogenous mixture?
its is a mixture where the components cannot be seen e.g. air
59
What is a heterogenous mixture
a mixture where the you can see the components e.g. vegetable soup a glass of water with coins in it
60
What is the difference between an element and a compond?
A compound can be broken down in to simpler substances, where as an elemant cant
61
Chemical reactions
* 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 ## Footnote 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
Reactants
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
Products
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
Metabolism
All chemical reactions that occur in the body
65
Energy
The capacity to do work 1. Potential energy (stored by matter) 2. kinetic energy (matter in motion)
66
Chemical energy
A form of potential energy stored in the bonds of compounds and molecules
67
Law of conservation of energy
Energy can be neither created or destroyed, it is converted to one form to another
68
Activation energy
The collision energy need to break the chemical bonds of reactants. Temperature and concentration of particles influence the change of collision
69
Catalysts
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
Types of chemical reactions
* Oxidation/reduction * Reversible * exchange * decomposition (catabolism) * Synthesis (anabolism)
71
Anabolism | (synthesis reaction)
* 2 or more atoms combining to form new and/or larger molecules * they absorb more energy than they release
72
Catabolism | (decomposition reaction)
* where larger molecules are split up into smaller molecules/atoms * uses more energy that they absorb
73
Exchange reactions
Consists of both * Synthesis reaction (anabolism) * decomposition reaction (catabolism
74
Reversible reactions
* when products can revert back to their original reactants * many of these reactions in the body require catalysts (enzymes)
75
Oxidation- Reduction reactions
* AKA Redox reactions * when one substance os oxidised and another is equally reduced at the exact same time * loss and gain of electrons
76
Oxidization
Loses electrons and released potential energy
77
Reaction
Gains electrons and gains potential energy
78
Displacement reactions
Movement of an atom from a compound to another atom to make a different compound Fe + CuSO4 -\> Cu + FeSO4
79
Combustion reaction
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
Mole
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
What are the three conditions required for a reaction to occur?
1. Collision 2. Orientation 3. Energy
82
What influences the chemical reaction rate?
* 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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