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A-level Chemistry > Electron Structure > Flashcards

Electron Structure Flashcards

1
Q

What charge does group one have?

A

1+ charge

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2
Q

What charge does group 2 have?

A

2+

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3
Q

What charge does Ag have?

A

+1

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4
Q

What charge does Za & Cd have?

A

2+

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5
Q

What charge does group 3 Al & Ga have?

A

3+

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6
Q

What charge does group 5 have?

A

-3

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7
Q

What charge does group 6 have?

A

-2

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8
Q

What charge does group 7 have?

A

-1

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9
Q

What is the formulae for nitrate?

A

No3 ^-

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10
Q

What is the formulae for carbonate?

A

CO3 ^2-

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11
Q

What is the formulae for sulphate?

A

SO4^2-

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12
Q

What is the formulae for hydroxide?

A

OH-

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13
Q

What is the formulae for ammonium?

A

NH4 ^+

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14
Q

What is the formulae for zinc?

A

Zn ^2+

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15
Q

What is the formulae for silver?

A

Ag+

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16
Q

What is the rule for predicting ionic formulae?

A

The charges have to equal and opposite.

So if you have one element with a +2 charge and one with a 1- charge you will have two of the element with the 1- charge

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17
Q

What is ionic bonding?

A

The electrostatic bonding between positive and negative ions

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18
Q

What is the maximum amount of electron that can fit in the first four shells?

A

2, 8, 18, 32

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19
Q

What are the 4 sub shells that an electron shell is split into?

A

-S

-P

-d

-f

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20
Q

What sub shell does shell one contain?

A

1s shell

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21
Q

What sub shells does shell 2 contain?

A

S shell & p shell

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22
Q

What sub shells does shell 3 contain?

A

S shell, d shell & p shell

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23
Q

How many orbitals does an S shell have?

A

Has 1 orbital

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24
Q

How many orbitals does a p shell have?

A

Has 3 orbitals

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25
Q

How many orbitals does a d shell have?

A

5 orbitals

26
Q

How many orbitals does shell d have?

A

7 orbitals

27
Q

How many electrons can an s shell hold?

A

2 electrons

28
Q

How many electrons can a p shell hold?

A

6 electrons

29
Q

How many electrons can a d shell hold?

A

10

30
Q

How many electrons can a F shell hold?

A

14 electrons

31
Q

What is the orbital shape of the s shell?

A

Spherical & electrons can move any where within the sphere

32
Q

What is the orbital shape of the p shell?

A

A dumbbell shape

33
Q

What is another word for the shell number?

A

Principal quantum number

34
Q

What is spin pairing?

A

It’s when 2 electrons occupy 1 orbital they spin in opposite direction

35
Q

What groups on the periodic table have an S shell for the outer electron?

A

Groups 1 & 2

36
Q

What groups in the periodic table have p shells as shells for the outer electron?

A

Groups: 3,4,5,6,0

37
Q

What group in the periodic table have d shells as there shell for the outer electron?

A

Transition metals

38
Q

What is the empirical formula?

A

It is the simplest whole number ratio for atoms of each element in the molecule

39
Q

What is the molecular formula?

A

It’s the actual number of atoms of each element in a compound.

40
Q

What are the steps to finding the empirical formula?

A

Step 1: write elements in a table

Step 2: write the masses of each element

Step 3: Divide by the Mr to get the moles - make sure moles are rounded to 3sfs

Step 4: divide moles by the smallest number to get a ratio. If it’s a decimal multiply by a suitable number to make it a whole number

41
Q

How do you find the empirical formula and molecular formula?

A

Step 1: write the elements in a table

Step 2: write the masses of the elements in a table

Step 3: divide by the mr to get the moles- make sure moles are rounded to 3SF

Step 4: divide the moles by the smallest number to get the ratio

Step 5: divide the Mr by the mass of the EF to find a factor to multiply by

42
Q

When do you round and multiply when working out the empirical formula?

A

You round if it’s no more than 0.1 away

And you multiply of the answer ends in:

.33= X3

.25=X4

.5=X2

43
Q

What is co-ordinate/dative covalent bonding?

A

A shared pair of electrons which have been provided by one of the bonding atoms only

44
Q

What is an example of co-ordinate/ dative covalent bonding?

A

Ammonium- nitrogen provides both electrons to one bonding hydrogen

45
Q

What are steps to working out the formula of a hydrated salt from mass data?

A

Step 1: find the mass of the water (difference in salts)

Step 2: find the moles of both the water and salt (mass/Mr)

Step 3: get the ratio of the salt to water by dividing the moles by the smallest

Step 4: use ratio to give you the formula of the salt

46
Q

What are the steps to find the formula of a hydrated salt from percentage composition data?

A

Step 1: set up a table of the salt and water

Step 2: calcínate the moles of each of them

Step 3: divide the moles by the smallest to get a ratio

Step 4: use the ratio to write the formula for the salt

47
Q

What are the steps into identifying the metal in a hydrated salt?

A

Step 1: find the mass of water produced

Step 2: work out the moles of water

Step 3: find the molar to molar rato between the anhydrous salt and water

Step 4: divide the moles of the water by its part in the ratio, to get the mole for the anhydrous salt

Step 5: using the moles of water work out the Mr of the anhydrous salt= mass/ moles

Step 6: subtract the Ar of the elements from the Mr calculated if the anhydrous salt to give you the Mr of X

48
Q

What is relative molecular mass (Mr)?

A

It’s the average mass of a molecule compared to 1/12 of the mass of an atom of carbon 12

49
Q

How do you calculate the Relative molecular mass (Mr)

A

Add up all the relative atomic mass values of all the atoms in the molecule

50
Q

What is relative formula mass?

A

The average mass of a formula unit compared to 1/12 of an atom of carbon 12

51
Q

How is relative formula mass worked out?

A

By adding up all the Ar units of the ions in the compound

52
Q

What is relative atomic mass?

A

Relative atomic mass is the weighted mean mass of an atom of an element compared to 1/12 of an atom of carbon-12

53
Q

How do you calculate relative atomic mass?

A

Sum of the number of atoms of an element
—————————-——————-
100

54
Q

What is relative isotopic mass?

A

The mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon 12

55
Q

How do you determine the relative atomic mass by mass spectrometry of an isotope?

A

R.A.M= total abundance of all isotopes
——————————————
100 (if it’s not %’s it’s the raw data above the lines)

56
Q

What is water crystallisation?

A

It’s when water is trapped within the structure of a crystal (hydrated salt

57
Q

What is a lattice?

A

A regular structure made up of the same basic units resorting over and over again

58
Q

Why can ionic substances only conduct electricity when molten or aqueous?

A

Because when molten or aqueous the ions are free to move as they are not held in sting positions by strong ionic bonds so they can now carry a charge

59
Q

Why do ionic substances have a hight melting/ boiling point?

A

Because the giant ionic lattices are held together by strong electrostatic forces which require a lot of energy to overcome

60
Q

Why are ionic substances soluble?

A

Because water molecules are polar part of the molecules have a negative charge and the other parts have positive charge- the water pulls the ions away from the lattice and cause it to dissolve

61
Q

What structures do metals form?

A

Giant metallic lattices

62
Q

What is covalent bonding?

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

A-level Chemistry (19 decks)

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