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Chemistry IGCSE > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

who invented the periodic table?

A

Dmitri Mendeleev

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2
Q

how many elements are there?

A

about 100 (118)

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3
Q

groups (vertical columns) indicate what?

A

the number of electrons in the outer shell of an element

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4
Q

what do the periods indicate?

A

the number of shells an atom has

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5
Q

why do elements of the same group have similar properties?

A

they have the same number of electrons in their outer shell

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6
Q

how many electrons do group 2 elements have in their outer shell?

A

2

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7
Q

group 1 elements are…

A

alkali metals

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8
Q

group 7 elements are…

A

halogens

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9
Q

group 0 elements are…

A

noble gases

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10
Q

what does the properties of elements depend on?

A

the number of electrons they have in their outer shell

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11
Q

how are electrons arranged in the shells?

A

they always fill the first shell first

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12
Q

how to figure out the electronic configuration of an atom?

A
  1. the atomic number indicates the number of protons and therefore electrons
  2. the period indicates the number of shells of an atom
  3. e.g nitrogen has 7 electrons and is found in period 2 so its electronic configuration is 2,5
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13
Q

find the electronic configuration of sodium using groups and periods

A
  • sodium is in period 3, so it has 3 shells occupied
  • the first 2 shells must be full (2,8)
  • sodium is in group 1 so it has 1 electron in its outer shell
  • 2,8,1
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14
Q

what can elements be classified as?

A

metals and non-metals

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15
Q

metals are on..

A

the left hand side of the periodic table

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16
Q

non metals are on the..

A

right hand side of the periodic table

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17
Q

where are metals and non-metals separated?

A

they are separated by a zig-zag going from Boron to Astatine

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18
Q

properties of metals

A
  • metals conduct electricity because they allow charge to pass through them easily
  • metal oxides are basic (they will neutralise acids)
  • metal oxides which dissolve will form solutions with a pH of more than 7
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19
Q

non-metals

A
  • poor conductors of electricity
  • non-metal oxides are acidic (they will neutralise bases)
  • they dissolve in water to form solutions with a pH of less than 7
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20
Q

group 0

A
  • noble gases are all inert, colourless gases
  • helium, neon, argon
  • inert - don’t react with much at all
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21
Q

why are noble gases inert?

A

it takes a lot of energy to add or remove electrons from a noble gas atom

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22
Q

ionic bonding

A
  • atoms lose or gain electrons and become ions
  • the oppositely charged ions are strongly attracted to one another by electrostatic attractions
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23
Q

simple ions form when…

A

atoms lose or gain electrons

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24
Q

negative ion

A

anion - gain electrons

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25
Q

positive ion

A

cation - lose electrons

26
Q

ions

A

are charged particles
- can be single atoms or groups of atoms

27
Q

the number of electrons lost or gained is the same as…

A

…the charge on the ion

28
Q

if two electrons are lost…

A

the charge is 2+

29
Q

if 3 electrons are gained…

A

the charge is 3-

30
Q

how do metals become ions?

A
  • they lose electrons to form positive ions (cations)
  • they are in group 1,2 and 3
31
Q

what type of ion do metals become?

A

cations (positive ions)

32
Q

what type of ion do non-metals become?

A

anions (negative ions)

33
Q

how do non-metals become ions?

A
  • they gain electrons to form negative ions (anions)
  • they are in group 5,6 and 7
34
Q

what structure do ionic compounds have?

A

a closely packed lattice structure

35
Q

how do group 1 elements form ions?

A

they lose 1 electron and become 1+ cations

36
Q

how do group 2 elements form ions?

A

they lose 2 electrons and become 2+ ions

37
Q

how do group 3 elements form ions?

A

they lose 3 electrons and become 3+ cations

38
Q

how do group 5 elements form ions?

A

they gain 3 electrons and become 3- anions

39
Q

how do group 6 elements form ions?

A

they gain 2 electrons and become 2- anions

40
Q

ammonium

A

NH₄⁺

41
Q

hydroxide

A

OH¯

42
Q

nitrate

A

NO3-

43
Q

sulfate

A

SO₄²-

44
Q

carbonate

A

CO₃²⁻

45
Q

hydrogen ion

A

H+

46
Q

silver ion

A

Ag+

47
Q

copper ion

A

Cu²⁺

48
Q

iron ion

A

Fe2+

49
Q

how many diatomic elements are there?

A

7

50
Q

what are the diatomic elements?

A
  • hydrogen
  • nitrogen
  • oxygen
  • fluorine
  • chlorine
  • bromine
  • iodine
51
Q

can ionic compounds conduct electricity?

A
  • they cant conduct electricity when they are solid
  • they are able when tehy are melted or dissolved
52
Q

why do ionic compounds have hight melting and boiling points?

A

the electrostatic attraction between the oppositely charged ions is very strong, and a lot of energy is needed to overcome the strong attraction

53
Q

covalent bonding

A

atoms bond by sharing pairs of electrons

54
Q

what is the force of attraction forms covalent bonds?

A

strong electrostatic attraction between the negatively charged shared electrons (bonding pair) and the positively charged nuclei of the atoms

55
Q

how are the elements arranged in the periodic table?

A

by atomic number

56
Q

what is the name given to the rows in the periodic table?

A

Periods

57
Q

what is the name given to the columns in the periodic table?

A

groups

58
Q

name the type of structure that ionic compounds have

A

giant ionic lattice

59
Q

which non-metal element can conduct electricity?

A

graphite

60
Q

why can graphite conduct electricity?

A

only 3 of each carbons 4 outer electrons are used in bonds, so each carbon atom has 1 electron that’s delocalised

61
Q
A

Chemistry IGCSE (4 decks)

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