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Chemistry > Atomic Structure And The Periodic Table > Flashcards

Atomic Structure And The Periodic Table Flashcards

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1
Q

talk to me about a proton.

A

relative mass of 1
relative charge +1

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2
Q

talk to me about a neutron.

A

relative mass 1
relative charge 0

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3
Q

talk to me about an electron.

A

relative mass very small
relative charge -1

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4
Q

what is a nuclear symbol?

A

used to describe atoms

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5
Q

what is mass number?

A

total number of protons and neutrons in an atom

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6
Q

What is atomic number?

A

Number of protons in an atom

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7
Q

What are elements?

A

Substances made up of atoms with the smae atomic number

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8
Q

What are isotopes?

A

Atoms with the same number of protons but different numbers of neutrons

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9
Q

What is relative atomic mass (RAM)?

A

The average mass number for an element

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10
Q

How do you work out RAM (A with a little r)?

A

Alittle r = sum of (isotope abundance x isotop mass number) / total abundance of all isotopes

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11
Q

What is a compound?

A

Substance formed from 2 or more elements chemically bonded together in fixed proportions

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12
Q

What is a molecule?

A

Particle containing 2 or more non-metal atoms bonded covalently. Molecules can be elements (if they only have one type of atom) or compounds

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13
Q

What does a chemical formula show?

A

The proportion of atoms of each element in a compound

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14
Q

What does a chemical equation show?

A

The overall change in a reaction

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15
Q

What is a mixture?

A

Substances made up of different elements or compounds that aren’t chemically bonded to each other. The chemical properties of a substance aren’t affected by neing part of a mixture.

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16
Q

What is filtration?

A

Seperates insoluble solids from liquids and solutions. It can be used to separate out a solid product, or purify a liquid by removinf insoluble impurities.

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17
Q

What is evaporation?

A

Separates soluble salts from solution.
Slowly heat your solution in an evaporating dish, then the crystals dry out as solvent evaporates

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18
Q

What is crystallisation?

A

Also separates soluble salts from solution.
Heat solution, but cool it when crystals start to form > large crystals form as solution cools > filter out crystals and leave to dry

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19
Q

What is simple distillation?

A

Put mixture in, heat it up, then the part with the lowest boiling point evaporates first. It vapourises and gets cooled and condenses in the condenser (water goes in and out) then you collect the pure liquid.

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20
Q

what is fractional distillation?

A

Mixture of liquids at the bottom, fractionating column is filled with glass rods. Liquids reach the top of the column when the temperature at the top matches their boiling point. They go through the condenser then the fractions get collected separately

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21
Q

what is the model of an atom at the start of the 1800s?

A

atoms described as solid spheres that can’t be divided

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22
Q

what is the model of an atom in 1897?

A

‘Plum pudding’ model - ball of positive charge containing small negative electrons

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23
Q

what is the model of an atom in 1909?

A

nuclear model - mass is concentrated in a positive nucleus with a cloud of electrons (and mostly empty space)

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24
Q

what is the model of an atom in 1913?

A

Bohr model - electrons orbit nucleus in fixed shells

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25
Q

what is the model of an atom in later experiments?

A

nucleus contains protons, which give it its positive charge

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26
Q

what is the model of an atom in 1932?

A

James Chadwick provided evidence that neutrons are neutral particles found in the nucleus

27
Q

Talk to me about electronic structure.

A

Electrons occupy shells (sometimes called energy levels)
They fill each shell up before occupying a new one, starting with the lowest energy
Lowest energy shells are closest to the nucleus

28
Q

how many electrons are allowed in the first shell?

A

2

29
Q

how many electrons are allowed in the second shell?

A

8

30
Q

how many electrons are allowed in the third shell?

A

8

31
Q

how many electrons are allowed in the fourth shell?

A

2 I think

32
Q

what is the last option for electronic structure?

A

calcium (2.8.8.2)

33
Q

talk to me about Mendeleev’s table.

A

before atomic structure was discovered, atomic weight was used to order elements.
In Mendeleev’s Table of Elements, the elements were grouped using their properties, instead of strictly following atomic weight.

34
Q

What was interesting about Mendeleev’s table?

A

he left gaps in the table to keep groups together (and later new elements that fitted the gaps were discovered)
he swapped some elements around in places where ordering by atomic weight didn’t fit the pattern (then isotopes were discovered and expalined why they couldn’t be arranged by atomic weight)

35
Q

what does the group number show?

A

the number of electrons in the outer shell

36
Q

what does the period number show?

A

the number of shells with electrons in

37
Q

what are metals?

A

elements that can form positive ions when they react

38
Q

what are non-metals?

A

elements that don’t generally form positive ions

39
Q

Talk to me about metals

A

get a full outer shell by losing electrons
more reactive when they lose electrons more easily
more reactive towards the bottom left of the periodic table

40
Q

talk to me about non-metals

A

get a full outer shell by gaining or sharing electrons
more reactive when they gain electrons more easily
more reactive towards the top right of the periodic table

41
Q

what are the properties of metals?

A

they appear shiny
they are strong but malleable
they have high melting and boiling points
they are good electrical and thermal conductors

42
Q

what are the properties of non-metals?

A

they appear dull
they are brittle
they have low melting and boiling points
they are poor electrical and thermal conductors

43
Q

what are transition metals?

A

metals in the centre of the periodic table

44
Q

what are 6 examples of transition metals?

A

1: Cr (chromium)
2: Mn (manganese)
3: Fe (iron)
4: Co (cobalt)
5: Ni (nickel)
6: Cu (copper)

45
Q

what are 3 differences of transition metals?

A

1: they have multiple ions (Fe 3+, Fe 2+ etc.)
2: they form colourful compounds
3: they can be good catalysts

46
Q

what are the alkali metals?

A

common name for the Group 1 metals

47
Q

what are the trends of group 1?

A

As you go DOWN the group:
Reactivity increases
Melting and boiling points decrease
relative atomic mass increases

48
Q

what are the 3 properties of the group 1 metals?

A

1: they’re much more reactive
2: they’re less dense and softer
3: they have lower melting points

49
Q

what is the metal + water reaction?

A

metal + water > metal hydroxide + hydrogen

50
Q

what is the metal + chlorine reaction?

A

metal + chlorine > metal chloride

51
Q

what is the metal + oxygen reaction?

A

metal + oxygen > metal oxide

52
Q

what are the group 0 elements?

A

non-metals with full outer shells

53
Q

talk to me about group 0.

A

their electronic structure is stab le so they are unreactive
All group 0 elements are colourless monatomic gases at room temperature
As you go down the group the boiling point increases

54
Q

what are the group 7 elements?

A

non-metals known as halogens

55
Q

what does fluorine look like?

A

yellow gas

56
Q

what does chlorine look like?

A

dense green gas

57
Q

what does bromine look like?

A

volatile red-brown liquid

58
Q

what does iodine look like?

A

dark grey solid or purple vapour

59
Q

what are fluorine, chlorine, bromine and iodine?

A

halogens

60
Q

what happens as you go down the group?

A

reactivity decreases
melting and boiling points increase
relative molecular mass increases

61
Q

are the halogens diatomic or monatomic?

A

diatomic

62
Q

what 2 ways can halogens react to fill their outer shell?

A

1: Sharing electrons - halogens form covalent bonds with other non-metals to form molecular compounds
2: gaining an electron - halogens form ionic compounds when they react with metals
- as they gain one electron, they form 1- ions called halides

63
Q

what can more reactive halogens do?

A

displace less reactive ones (eg, Cl2 + 2KBr > Br2 + 2KCl)

Chemistry (11 decks)

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