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Chemistry > Atoms, ions and compounds > Flashcards

Atoms, ions and compounds Flashcards

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1
Q

What is relative atomic mass?

A

The weighted mean mass of one atom of an element compared to the mass of 1/12 of the mass of an atom in carbon-12

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2
Q

What is the relative isotopic mass?

A

The weighted mean mass of an atom of an isotope compared to the mass of 1/12 of the mass of an atom in carbon-12

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3
Q

What is ionisation energy?

A

The amount of energy required to remove the most loosely held electron from one mole of gaseous atoms to produce one mole of gaseous atoms each with a +1 charge

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4
Q

What is the charge on a proton, neutron and electron?

A

Proton: +1
Neutron: 0
Electron: -1

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5
Q

What are ionisation energies measured in?

A

KJ/mol

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6
Q

What is the relative mass of protons, neutrons and electrons?

A

Protons: 1
Neutrons: 1
Electrons: 0.0005

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7
Q

What are the orbital types?

A

S, P, D or F

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8
Q

What is an isotope? What is it in terms of protons and neutrons?

A

A differing form of the same element. It has the same number of protons and a different number of neutrons.

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9
Q

What is the maximum number of electrons in the S orbital?

A

2

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10
Q

What is the maximum number of electrons in P orbital?

A

6

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11
Q

What is the maximum number of electrons in D orbital?

A

10

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12
Q

What is the filling order of electrons in energy levels?

A 
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
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13
Q

What are the rules when electrons are pairing?

A

Electrons enter one at a time in an orbital before they pair up

Electrons enter the lowest available energy level

One arrow must be up and one must be down as they spin in opposite directions

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14
Q

What is an orbital?

A

A place in the atom which the electrons are 95% most likely to be found

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15
Q

What does the group determine about an atom?

A

The number of electrons there are in its outer shell

E.g: group 1 elements have 1 electron

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16
Q

What do the periods determine about elements?

A

The number of shells the element has

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17
Q

Do all elements have ionisation energy?

A

YES

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18
Q

If there was an electronic configuration ending in 4 or 9 in the D orbital, what is the rule?

A

One electron is promoted from S to D to make D either equal to 5 or 10

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19
Q

Why does the rule about D orbital being 4/9 affect the stabilisation of the atom?

A

There is a more stable arrangement if an electron from S is promoted to D to give 6 paired electrons with lower repulsion

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20
Q

What is a sub-atomic particle?

A

A particle IN an atom:
Proton
Neutron
Electron

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21
Q

Why is there an increase of ionisation energy between F and Ne in the periodic table?

A

There are more electrons in Neon than Fluorine so there are also more protons. This means there is a stronger force of attraction and therefore more energy is required to remove an electron.

22
Q

What is an isotope in terms of subatomic particles?

A

A differing form of the same element. There are the same number of protons and different numbers of neutrons

23
Q

Do isotopes have the same chemical properties? Why?

A

They do have the same chemical properties as they have the same electron arrangement

24
Q

What are the 4 main factors affecting ionisation energy?

A
  • Charge in the nucleus (the higher the number of protons and electrons, the stronger the attraction)
  • The distance from the nucleus (attraction falls rapidly with distance)
  • Shielding (Number of inner electrons between outer electrons and nucleus - if there are more, the attraction is ‘shielded’ by inner energy levels)
  • Lone or paired electron (repulsion of electrons means paired electrons are removed more easily)
25
Q

How is relative atomic mass calculated?

A

(% isotope 1 x RFM ) + (% isotope 2 x RFM) + (%isotope3 x RFM)

Divided by

Total % of isotopes

26
Q

What is valency?

A

The number of electrons an atom loses or gains

27
Q

What are the steps in order to calculate formulae using Valencies?

A

Write the valency above the element symbol

Cross over

Write out in full underneath

Balance otherside

28
Q

In Valencies, what is the rule with elements in group 7?

A

They always go in pairs

E.g: O2

29
Q

Acronym for shapes of electrons?

A 
Lonely
Tony
Pulls
Tiny 
Teeth
But 
(It's)
Offensive 
Vicky 
Parker 
Shoots 
Pretty 
Lions
30
Q

Give the 3 types of bonding and what they bond

A

Ionic - metal and non-metal
Covalent - both non-metal
Metallic - both metal

31
Q

What is the difference between inter/intramolecular forces?

A

Inter - between molecules

Intra - within molecules

32
Q

What are the types of intermolecular forces in order from weakest to strongest?

A

Van Der waals
Dipole-dipole
Hydrogen bonding

33
Q

What is electronegativity?

A

The ability of an atom to attract a pair of electrons to itself

34
Q

Why is second ionisation energy greater than first ionisation energy?

A

More energy is required to remove an electron from a positively charged ion

35
Q

How can you determine which ‘block’ an element is in?

A

Write out the electronic configuration. Which ever orbital (S, P or D) it ends on is its block

36
Q

What is the difference between a symbol equation for first ionisation energy and second?

A

The element which is being represented starts with an additional positive charge (x-1)

37
Q

Why do isotopes have the same chemical properties?

A

Isotopes have the same number of electrons and thus the same chemical helical properties

38
Q

What is dative covalent bonding?

A

A dative covalent bond is a covalent bond (a shared pair of electrons) in which both electrons come from the same atom.

39
Q

What are the anomalous properties of water?

A

High surface tension

Specific heat capacity

40
Q

What is ionic bonding?

A

The attraction between oppositely charged ions. The electrostatic attractions between the positive and negative ions hold the compound together.

41
Q

What is covalent bonding?

A

The sharing of a pair of electrons between two non-metals

42
Q

How is volume calculated?

A

Moles

Divided by

Concentration/molarity

43
Q

How is volume at RTP calculated?

A

Moles x 24

44
Q

How is dm^3 converted to cm^3?

A

/1000

45
Q

How are oxidation numbers calculated?

A

Calculate the valency

Add to whatever is needed to make the overall charge 0. Whatever number this is is the oxidation number

46
Q

Give the formulae of ammonium

A

NH4+

47
Q

Give the formulae for hydroxide

A

OH-

48
Q

Give the formulae for carbonate

A

CO3^2-

49
Q

Give the formulae of sulfate

A

SO4^2-

50
Q

Give the formulae for nitrate

A

NO3^-

51
Q

What is meant by the term mole?

A

The amount of a substance which has the same number of particles as there are in 12g of carbon-12

Chemistry (10 decks)

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