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Chemistry > Unit 2 - Mr Shah > Flashcards

Unit 2 - Mr Shah Flashcards

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1
Q

Define Relative Isotopic Mass

A

The mass of an atom of an isotope compared with 1/12 of carbon -12

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2
Q

Define an Isotope

A

Atoms of the same element with the same number of protons but a different number of neutrons and different masses

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3
Q

Define An Orbital

A

The region where an electron is

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4
Q

Define First Ionisation Energy

A

The energy required to remove one mole of electrons (to infinity) from one mole of gaseous atoms to form one mole of gaseous positive ions

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5
Q

Define a Covalent Bond

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atom

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6
Q

Define a Dative covalent bond

A

A shared pair of electrons in which ONLY one of the bonded atoms provides the bonded pair

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7
Q

Define Ionic Bonding

A

The electrostatic attraction between positive and negative ions

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8
Q

Define electronegativity

A

A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond

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9
Q

Define a Dipole

A

A separation in electrical charge so that one atom of a polar covalent bond, or one end of a polar molecule, has a small positive charge, and the other has a small negative charge

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10
Q

Define a permanent Dipole

A

A small charge difference that doesn’t change across a bond, with partial charges on the bonded atoms: resulting in the bonded atoms having different electronegativities.

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11
Q

What is the name and angle of a compound with 2 electron pairs?

A

Linear, 180 degrees

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12
Q

What is the name and angle of a compound with 3 electron pairs?

A

Trigonal Planar, 120 degrees

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13
Q

What is the name and angle of a compound with 4 electron pairs?

A

Tetrahedral, 109.5 degrees

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14
Q

What is the name and angle of a compound with 5 electron pairs?

A

Trigonal Bipyramidal, 90 and 120 degrees

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15
Q

What is the name and angle of a compound with 6 electron pairs?

A

Octahedral, 90 degrees

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16
Q

With what 3 atoms does hydrogen bonding take place?

A

N,F and O

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17
Q

What is the relative mass and charge of a proton?

A

1 and +

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18
Q

What is the relative mass and charge of a neutron?

A

1 and 0 (neutral)

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19
Q

What is the relative mass and charge of an electron?

A

1/2000 and -

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20
Q

What do we use a mass spectrometer for?

A

To weigh atoms in a compound to find their abundance

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21
Q

What is the equation for Relative atomic mass from a mass spectrometer?

A

the sum of(relative atomic mass x abundance) / 100

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22
Q

How do you find the maximum number of electrons on each shell?

A

2n^2 where n is the shell number

23
Q

Name the full order up to 4f of the sub-shells

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f

24
Q

How many electrons does an s sub-shell hold?

A

2

25
Q

How many electrons does a p sub-shell hold?

A

6

26
Q

How many electrons does a d sub-shell hold?

A

10

27
Q

How many electrons does an f sub-shell hold?

A

14

28
Q

What are the exceptions to the rule and how are they different?

A

Cr as it goes 4s^1, 3d^5 instead of 4s^2, 3d^4
Cu as it goes 4s^1, 3d^10 instead of 4s^2, 3d^9

This is because the 4s and 3d levels are very close in energy.

29
Q

How do you draw short structures of electronic arrangements?

A

Use noble gases. E.g. Lithium is 1s^2, 2s^1

but [He] has an electronic arrangement of 1s^2 so we can draw it as [He] 2s^1

30
Q

What 3 factors affect the ionisation energy?

A
  • Amount of shielding by shells
  • Distance from the positively charged nucleus (atomic radius)
  • Number of protons
31
Q

Why going across periods is there sometimes a dip in ionisation energy, eg. from Neon to sodium?

A

Either:

  • It’s an electron in it’s own sub-shell so easier to remove
  • It’s an electron with another electron in an orbital so they repel
  • The electron moves into the next shell, so shielding is less and distance from the nucleus is more
32
Q

Write the equation for the first ionisation energy of Li

A

Li —> Li+ + e-

g) (g

33
Q

Write the equation for the first ionisation energy of Al

A

Al —> Al+ + e-

s) (s

34
Q

Write the equation for the second ionisation energy of Li

A

Li+ —> Li2+ + e-

g) (g

35
Q

Name the giant covalent molecules

A

Diamond and Graphite

36
Q

Name a few properties of Metallic compounds

Refer to M.P , conductivity and strength

A

High M.P - Ease of separation depends on density of electron cloud and ionic charge
Malleable and Ductile - The electron clouds BIND ions together
Does conduct - There are mobile/free electrons that can carry a charge
GIANT STRUCTURE
Electrostatic attraction between postive and negative ions (put in exam)

37
Q

Name a few properties of simple covalent compounds

Refer to B.P , conductivity and solubility

A

Low B.P - Only have WEAK Van der Waals forces which means little energy is required to break them
Doesn’t conduct - No free electrons
Solubility - Tends to be in organic solvents than water
ATTRACTION BETWEEN MOLECULES INCREASE AS THE MOLECULES GAIN ELECTRONS

38
Q

Name a few properties of ionic compounds

Refer to M.P ,Strength, conductivity and solubility

A

Very high M.P - Strong electrostatic attraction
Very Brittle - Any distortion leads to layers moving and similar ions being next to each other, which repel and crack the crystal
Doesn’t conduct when solid - ions held in a lattice
DOES conduct when MOLTEN or in AQUEOUS solution - Has free electrons
Only soluble in water

39
Q

Name a few properties of giant covalent structures

Refer to M.P ,Conductivity and strength

A

Very High M.P - Lattice is made up of large number of covalent bonds, which must all be broken
Doesn’t conduct - No free electrons
BUT… Graphite does conduct as each C is only uses 3 outer electrons to bond. The other can carry a charge
Strength - Diamond is a hard, rigid structure
Graphite is soft as it is in layers which can slide

40
Q

What is the formula of ammonia?

A

NH3

41
Q

What are the formulas of a nitrate and a nitrite

A

No3- and No2-

42
Q

What are the formulas of a sulphate and a sulphite?

A

So4 2- and So3 2-

43
Q

What do we use to predict ionic formula?

A

The group of the element
Eg. if an element is in group 2, the charge is 2+
if an element is in group 7, the charge is 1-

44
Q

What is the pair of electrons called that we use in dative covalent bonds?

A

A lone pair

45
Q

What must we look for when determining the strength of ionic bonds?

A

Charge and atomic radius (smaller is stronger)

46
Q

What must we look for when determining the strength of metallic bonds?

A

The atomic radius (smaller means stronger), charge and the number of delocalised electrons

47
Q

What is the most electronegative element?

A

Fluorine

Cl, N and O are very electronegative aswell

48
Q

What happens to the electron pair when an element is a lot more electronegative?

A

They move to the more electronegative element, and so it gets a partial negative charge

The bond would then be POLAR

49
Q

Would CCL4 be polar?

A

No as it is symmetrical

50
Q

Would Cl2 be polar?

A

No as the 2 chlorines have the same pulling power

51
Q

Can permanent dipole-dipole interaction happen ONLY in ionic or covalent bonds?

A

Covalent molecules, e.g HCl

52
Q

How does the number of electrons affect Van der Waals forces?

A

More electrons = Stronger Van der Waals forces

53
Q

Name an anomalous property of water

A

Ice is less dense than water (H bonds hold water molecules apart)
Water has a RELATIVELY high M.P/B.P
Relatively high surface tension

54
Q

Define Relative Atomic Mass

A

The weighted mean mass of an atom compared with 1/12 of the mass of carbon -12

Chemistry (9 decks)

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