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Chem > Chap 4 - periodic table - Mendeleev, G1, G7, G0, transition metals > Flashcards

Chap 4 - periodic table - Mendeleev, G1, G7, G0, transition metals Flashcards

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1
Q

which group is missing from Mendeleev’s table

A

group 0

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2
Q

why was group 0 harder for Mendeleev to discover

A

they are unreactive

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3
Q

name for group 1

A

alkaline metals

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4
Q

name for group 2

A

alkaline earth metals

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5
Q

name for group 7

A

halogens

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6
Q

name for group 0

A

noble gases

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7
Q

2 ways Mendeleev’s table is more useful than Lavoisier’s table

A

-left gaps for missing elements that weren’t discovered yet
-can use to work out electronic structure

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8
Q

why did Mendeleev leave gaps in his table

A

he believes that there were elements that had not been discovered yet

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9
Q

Explain how the modern periodic table was arranged in terms of their atomic strucutre

A

arranged in:
-groups - no. electrons in valance shell
-periods - no. occupied shells
-elements in order of proton number

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10
Q

explain how the position of the atoms are linked to the electronic structure of the atom

A

-groupis number of electrons in the outer shell
-across is period based on number of occupied shells
-each successive atom has one more electron

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11
Q

electronic structure of G1

A

1 e- in out shell

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12
Q

electronic structure in G7

A

7 e- in out shell

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13
Q

electronic structure of G0

A

full outer shell of e-

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14
Q

electronic structure of transition metals

A

forms differently charged ions

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15
Q

Trends in G1 as you go down

A

reactivity- up
density- up
melting point- down

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16
Q

Trends in G7 as you go down

A

reactivity- down
density- up
melting point- up

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17
Q

Trends in G0 as you go down

A

reactivity- unreactive
density- up
melting point- nul

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18
Q

Trends in transition metals as you go down

A

reactivity- unreactive
density- more dense than G1
melting point- high, except mercury

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19
Q

conductivity of G1

A

yes

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20
Q

conductivity of G7

A

no

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21
Q

conductivity of G0

A

no

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22
Q

conductivity of transition metals

A

yes

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23
Q

what are G7 molecules

A

diatomic

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24
Q

what are G0 atoms

A

monoatomic

25
Q

Where are G1 stored and why

A

in oil so they do not oxidise or react with water

26
Q

How do you test for hydrogen

A

Put a lit splinter next to the gas and you will hear a squeaky pop

27
Q

What is the G1 and G2 on the ph scale

A

basic

28
Q

How do you know G1 is basic

A

it turns purple under universal indicator after reacting with water.

29
Q

What type of molecules do ionic and covalent bonding form in terms of ph scale

A

ionic- basic compounds
covalent- acidic compounds

30
Q

Alkaline metal + water -> ?

A

Metal hydroxide + hydrogen

31
Q

Alkaline metal + oxygen->?

A

metal oxide

32
Q

what type of flame is produced when potassium reacts with water

A

lilac

33
Q

define precipitate

A

solid product

34
Q

what colour is copper usually

A

blue

35
Q

are nitrogen, oxygen and hydrogen diatmoic

A

yes

36
Q

colour and state of chlorine, bromine, iodine at room temperature

A

chlorine- pale yellow- green gas
bromine- red- brown liquid
iodine- grey- black solid

37
Q

most reactive metal in G7

A

Flourine

38
Q

how does iodine change state

A

sublimation, solid to gas

39
Q

properties of G1

A

-good conductors of electricity
-good conductors of heat
-soft metals

40
Q

What is true about displacement reactions

A

the more reactive element will displace the less reactive element from the compound

41
Q

what is a compound with halogen called

A

halide

42
Q

What colourd compound do G1 form when bonded with non- metals

A

white coloured

43
Q

do transition metals form colourless compounds

A

no

44
Q

what are transition metals used as

A

catalyst

45
Q

what are catalyst used for

A

to speed up a chemical reaction

46
Q

Why do G1 get more reactive as you go down

A

the outer electron is further from the nucleus so the shielding effect is greater, meaning it is easier to lose an electron

47
Q

Why do G7 get more reactive as you go up

A

the outer shell of electrons is closer to the nucleus so the shielding effect is less, meaning it is easier to gain an electron

48
Q

2 uses of noble gases

A

argon in lamps, helium in balloons

49
Q

What happens to the structure of an element across the period table

A

giant metallic (eg. Li) - giant covalent (eg. C) - simple covalent (eg. Ne)

50
Q

5 properties of transition metals

A

-high melting point
-high density
-good conductors of heat and electricity
-form coloured compounds
-low volatility

51
Q

What happens to colour as you go down G7

A

gets darker

52
Q

trend in metallic character across a period

A

metal to non- metal

53
Q

What happens to the structure of an element across a period?

A

Giant metallic (e.g. Li) - giant covalent (e.g. C) - simple molecular (e.g. Ne)

54
Q

what is the colour of a halogen ion

A

colourless

55
Q

what is the difference between a halogen ion and a halogen itself (not in a compound) in terms of colour

A

halogen ion- colourless
halogen- has colour

56
Q

what is the colour of the solution when G1 metals react with halogens

A

colourless solution

57
Q

what is the colour of iodine and bromine when aqueous

A

bromine- orange
iodine- brown

58
Q

trends in group 7

A

-Reactivity decreases
-melting point increases
-they become darker
-density increases

59
Q

describe G0

A

unreactive monoatomic gases

Chem (12 decks)

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