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new science > C2 atoms, elements and compounds > Flashcards

C2 atoms, elements and compounds Flashcards

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Biology 101 flashcards
1
Q

define element

A
  • chemical substance
  • cant be broken down into simpler substances
  • composed of one type of atom only
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2
Q

define compounds

A
  • substance made of 2 or more elements
  • chemically bonded together
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3
Q

define mixture

A
  • 2 or more chemical substances found together
  • not chemically bonded
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4
Q

describe the structure of an atom

A
  • central nucleus (containing neutrons and protons)
  • surrounded by electrons in shells
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5
Q

relative charge of a proton

A

+1

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6
Q

relative mass of a proton

A

1

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7
Q

relative mass of a neutron

A

1

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8
Q

relative charge of a neutron

A

0

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9
Q

relative mass of an electron

A

negligible

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10
Q

relative charge of an electron

A

-1

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11
Q

define proton number

A

number of protons in nucleus of an atom

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12
Q

another word for proton number

A

atomic number

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13
Q

define mass number

A

total number of protons and neutrons in nucleus of an atom

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14
Q

another word for mass number

A

nucleon number

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15
Q

max number of electrons in innermost shell

A

2

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16
Q

max number of electrons in shells (except innermost)

A

8

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17
Q

what are elements in group VIII known as

A

noble gases

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18
Q

electrons in outer shell of group VIII?

A

full

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19
Q

correlation between group number and number of outer shell electrons

A

they are equal

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20
Q

correlation between occupied electron shells and period number

A

equal

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21
Q

define isotopes

A
  • different atoms of same element
  • same number of protons but different numbers of neutrons
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22
Q

why do isotopes of the same element have the same chemical properties

A
  • same number of electrons
  • therefore same electronic configuration
23
Q

what is the force which occurs in a chemical bond

A

electrostatic force

24
Q

why does chemical bonding occur

A

so all atoms involved achieve an electronic configuration with a full valence shell, which is highly stable

25
Q

what is a cation

A

positive ion

26
Q

what is an ion

A
  • electrically charged particle
  • formed when atom loses/gains electrons
27
Q

what is an anion

A

a negative ion

28
Q

what is an ionic bond

A
  • strong electrostatic attraction
  • between oppositely charged ions
29
Q

properties of ionic compounds:

A
  • high melting/boiling point
  • good electrical conductor when aqueous/molten
  • poor electrical conductor when solid
  • generally soluble in water
30
Q

what is the structure of ionic compounds

A

giant lattice structure
- regular arrangement
- alternating positive and negative ions

31
Q

why does an ionic compound form a lattice structure

A
  • electrostatic forces of attraction between alternating oppositely charged ions
  • act in all directions
  • to make giant 3d lattice
32
Q

why is the melting/boiling point of ionic compounds high

A
  • strong electrostatic force of attraction in all directions
  • more thermal energy required to break bonds and turn substance to liquid
33
Q

how does charge on ion impact melting point of ionic compound

A

higher charge on ions, higher the melting point

34
Q

why cant ionic compounds conduct electricity while solid

A
  • ions in giant 3d lattice unable to move freely
  • because held tg by strong electrostatic forces of attraction
  • ions are unable to carry charge
35
Q

why can ionic compounds conduct electricity while molten/aqueous

A
  • ions are able to move
  • carry a charge
36
Q

how is a covalent bond formed

A
  • pair of electrons is shared between 2 atoms
  • leading to noble gas electronic configurations
37
Q

properties of simple molecular compounds

A
  • low melting/boiling points
  • poor electrical conductivity
38
Q

why do simple molecular compounds have low melting/boiling points

A
  • intermolecular forces between molecules weak
  • not much energy needed to overcome
39
Q

relationship between mass of molecules and boiling/melting point

A
  • larger molecules have greater number of weak intermolecular forces
  • therefore require more energy to separate molecules
  • therefore melting/boiling point higher
40
Q

why are simple molecular compounds poor electrical conductors

A
  • do not have any charged particles which can move through structure
  • therefore charge does not flow
41
Q

what is the structure of diamond

A
  • each carbon atoms shares 1 electron with 4 other carbon atoms
  • to make giant repeating network of covalently bonded carbon atoms
42
Q

uses of diamond and why

A
  • cutting tools
  • extremely hard substance
43
Q

why is diamond so hard

A

made up of many strong covalent bonds in a giant structure

44
Q

what is the structure of graphite

A
  • comprised of layers
  • each layer made up of carbon atoms, each bonded to 3 other atoms
  • delocalised electrons can move freely across layers
  • stacks of layers held tg by many weak intermolecular forces
45
Q

define allotrope

A

alternative forms of an elemental substance

46
Q

uses of graphite and why

A
  • lubricant (layers can slide over each other)
  • electrode (good conductor of electricity)
47
Q

why can the layers in graphite slide over each other

A
  • layers have weak intermolecular forces holding tg
  • forces are weak
48
Q

why is graphite a good conductor of electricity

A
  • has delocalised electrons
  • which can move freely throughout structure and carry electric current
49
Q

describe metallic bonding

A
  • electrostatic attraction
  • between positive ions in giant metallic lattice and sea of delocalised electrons
50
Q

properties of metals

A
  • good electrical conductivity
  • malleable
  • high melting/boiling point
51
Q

why do metals have high melting/boiling point

A
  • metallic lattice held tg by strong electrostatic forces of attraction
  • a lot of energy needed to separate metal atoms
52
Q

why are metals good electrical conductors

A
  • delocalised electrons in metallic lattice
  • free to move throughout structure
53
Q

why are metals malleable

A
  • regular layers, practically identical (all ions same size and distance)
  • when force applied, layers are able to slide past other layers
54
Q

why will aluminium have a higher conductivity than sodium

A
  • one aluminium atom delocalises 3 electrons in metallic bonding
  • compared to only 1 in sodium
  • more delocalised electrons = higher conductivity

new science (41 decks)

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