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Nat 5 chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

how many elements are there

A

118

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2
Q

how are the elements get arranged in groups

A

according to how many are in the outer most energy level

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3
Q

describe alkali metals

A

VERY reactive
soft
react with water
react with oxygen

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4
Q

describe transition metals

A

hard and dense
less reactive
used in catalysts
form coloured compounds

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5
Q

describe the halogens

A

diatomic elements
all toxic
chlorine used to sterilise swimming pools

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6
Q

describe nobel gases

A

least reactive
DO NOT REACT AT ALL

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7
Q

what is the centre of the atom called and what does it contain what’s its charge

A

its called the nucleus and contains protons and neutrons and is positively charged

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8
Q

what circles round the atom and what is its charge

A

the electrons circle round and are negatively charged

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9
Q

how is the atom neutral

A

its neutral because the number of positively charged protons cancels out the negatively charged electrons

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10
Q

what is the top number mean in nuclide notation

A

the top number is the mass number

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11
Q

what is the bottom number in nuclide notation and what does it represent

A

its the atomic number and represents the number of protons and electrons

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12
Q

what are isotopes

A

isotopes are atoms of the same element have the same atomic number but diffrent mass numbers

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13
Q

how do you calculate the relative atomic mass

A

(mass of isotopes 1 x %) + (mass isotopes 2 x %) divide by 100

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14
Q

what is the electron arrangement for sodium

A

2,8,1

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15
Q

why do elements in a group have similar chemical properties

A

because they have the same number of outer electrons

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16
Q

what is an ion

A

an ion is where an atom gains or loses electrons and charged particles which are ions are formed

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17
Q

what happens if an atom gains an electron

A

it becomes a negatively charged ion

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18
Q

what happens if an atom loses an electron

A

it becomes a positively charged ion.

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19
Q

do metals gain or lose electrons

do non-metals gain or lose electrons

A

metals always lose to become positively charged

non-metals always gain to become negativly charged

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20
Q

why do atoms lose or gain electrons

A

its so they achieve a full outer most energy level.

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21
Q

what are atoms joined by

A

atoms can be joined by bonds

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22
Q

if the bonded atoms are the same what is it

A

its a molecule of an element

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23
Q

what is a diatomic molecule

A

diatomic molecules are made up of only two atoms

24
Q

what are the seven diatomic elements

A

Oxygen
Flurine
Chlorine
Nitrogen
Hydrogen
Iodine
Bromine

25
Q

why do atoms form bonds

A

in order to achieve a most stable outer electron arrangement (a full outer shell)

26
Q

what is a covalent bond

A

two positive nuclei held together by their common attraction for the shared pair of negative electrons

27
Q

what are covalent bonds formed from

A

they are usually formed between two non-metal elements

28
Q

are covalent bonds strong

A

they are extremely strong and need lots of energy to break

29
Q

what are bonding diagrams

A

they are simplified pictures of an atoms outer electrons

30
Q

how do atoms form bonds

A

using the electrons in their outer most energy level

31
Q

what molecular would hydrogen oxide be

A

angular

32
Q

what are covalent networks

A

gains network structures held together by strong covalent binds

33
Q

give an example of chemical formula

A

H2O

34
Q

what is the formula to work out the valency

A

Symbol
Valency
Swap
Divide
Formula

35
Q

what would be the valency for Magnesium chloride

A

Mg Cl
2 1
1 2
1 2
MgCl2

36
Q

what are the Roman numerals from 1-7

A

1 - I
2 - II
3 - III
4 - IV
5 - V
6 - VI
7 - VII

37
Q

what is the valency for iron(II)chloride

A

S - Fe Cl
V - 2 1
S - 1 1
D - 1 1
F - FeCl2

38
Q

what are the prefixes for numbers 1-7

A

1 - mono
2 - di
3 - tri
4 - tetra
5 - penta
6 - hexa
7 - heat

39
Q

what would thee answer be t o carbon monoxide

A

CO

40
Q

when does ionic bonding occur

A

between a metal and non-metal
between an positive and negative ion

41
Q

what is an ionic lattice

A

a giant arrangement of ions held together by electrostatic attraction (ionic bonds)

42
Q

what are 3 things you know about ionic lattice

A

it consists of millions of ions held together by ionic bonds

lots of energy required to break the bonds

always solid at room temputure

43
Q

what is the ionic formula for Hydrogen fluride

A

S - H. F
V - 1. 1
S - 1. 1
D - 1. 1
F - HF
I - H+F-

44
Q

what are the charges on the ions for numbers 1-7

A

1 - +
2 - 2+
3 - 3+
4 - /
5 - (-)
6 - 2-
7 - 3-

45
Q

what is a conductor of electricity

A

it allows electric current to flow through

46
Q

what is a non-conductor of electricity

A

it does not allow electrical current to flow through

47
Q

are metals elements conductor or not

A

they do conduct

48
Q

do non-metals conduct

A

NO

49
Q

what is metallic bonding

A

the outer electrons of metal atoms are not attached to a particular atom and are free to move around. THEY ARE DELOCALISED

50
Q

why do metals conduct electricity

A

because electrons can flow through them

51
Q

what is covalent bonding

A

where electrons are not free to ,one around and there is no conduction of electricity

52
Q

what is conductivity in non-metals

A

non-metals do not have charged particles which can move therefore they do not conduct electricity

53
Q

do covalent compounds (solid, liquid, gas) conduct electricity

A

NO
because they are not free to move around

54
Q

do ionic compounds electricity at all

A

yes when dissolved in water or when molten

55
Q

what happens when melting ionic compounds

A

it breaks down the lattice and allows the ions to move.

Nat 5 chemistry (1 decks)

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