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Chemistry Year 1 > Elements Of Life > Flashcards

Elements Of Life Flashcards

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1
Q

What is atomic number?

A

The number of protons in an atom

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2
Q

What is mass number?

A

The total number of protons and neutrons

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3
Q

What is relative atomic Mass?

A

Mean weighted mass of an Atom of an element compared with 1/12 Mass of an atom of carbon-12

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4
Q

What is relative molecular Mass?

A

Mean weighted mass of a molecule compared with 1/12 Mass of an atom of carbon-12

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5
Q

What is relative formula Mass?

A

Sum of all mean weighted masses of all atoms in the formula of a compound compared with 1/12 the Mass of an atom of carbon-12

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6
Q

What is relative isotopic Mass?

A

Mass of an atom isotope compared with 1/12 the Mass of an atom of carbon-12

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7
Q

What is the mole?

A

The amount of substance containing as many particles as there are atoms in 12g of carbon-12. 1 mole = 6.02x10^23 items

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8
Q

How is percentage yield calculated?

A

Percentage yield= (actual yield/ theoretical yield) x100

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9
Q

What shape are s and P orbitals?

A

S= spherical, p= dumb-bell

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10
Q

How are electrons arranged in orbitals?

A

Electrons fill from the lowest energy level first. Electrons will occupy orbitals by themselves end will only pair if no other energy orbitals are available.

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11
Q

What is fusion and what conditions are needed?

A

When two lighter nuclei collide and combine to form a heavier nucleus, releasing energy.
Very high temperature and pressure.

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12
Q

What is covalent bonding?

A

The electrostatic attraction between a par of shared electrons and two positive nuclei

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13
Q

Why are ion’s substances only conductive when dissolved?

A

When they are dissolved the ions are free to move so can carry a charge

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14
Q

Why do covalent and ionic lattices have high melting points?

A

Both lattices contain atoms that have strong and regular bonds around them which require a lot of energy to overcome.

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15
Q

2 bonding groups
2 lone pairs

A

Non-linear
104.5°

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16
Q

3 bonding groups
O lone pairs

A

Trigonal planar
120°

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17
Q

2 bonding groups
0 lone pairs

A

180°
Linear

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18
Q

2 bonding groups
1 lone pair

A

Non-linear
120°

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19
Q

4 bonding groups
0 lone pairs

A

Tetrahedral 109°

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20
Q

3 bonding groups
1 lone pair

A

Pyramidal
107°

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21
Q

5 bonding groups
0 lone pairs

A

Trigonal bipyramidal
120° + 90°

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22
Q

6 bonding groups
0 lone pairs

A

Octahedral
90°

23
Q

How do different numbers of bonded and lone pairs produce different shapes in molecules?

A

Lone pairs repel more than bonded groups

24
Q

What is ionic bonding?

A

The electrostatic attraction between ions of opposite charge

25
Q

What is first ionisation enthalpy?

A

The enthalpy change that occous when one mole of electrons is removed from one mole of gaseous atoms

26
Q

What does the group number represent?

A

Number of electrons in outer energy level

27
Q

What does the period number represent?

A

Number of energy levels in the atom

28
Q

Why does first ionisation enthalpy increase across a period?

A

Same number of electron shells but number of protons in the nucleus increases therefore increasing force of attraction between nucleus and outer electrons

29
Q
A

-

30
Q

What is molecular formula?

A

Actual number of atoms in a molecule

31
Q

What is empirical formula?

A

Smallest whole number ratio of atoms in a compound

32
Q

How do you calculate water of crystalisation?

A

Calculate number of moles of water and anhydrous salt (mass/mr= moles)
Divide moles of water by moles of anhydrous salt to get x

33
Q

How do you calculate % atom economy?

A

% atom economy = (Mr of desired product/Mr of all product)x 100

34
Q

What is an acid?

A

An H+ donor

35
Q

How do you prepare a standard solution of acid (6 marks)

A
36
Q

Define electronegativity

A

Ability of an atom to attract electrons in a covalent bond

37
Q

Define metallic bonding.

A

Electrostatic attraction between metal cations and a sea of delocalised elections

38
Q

How do the charge densities of group 2 ions affect the thermal stability of their carbonates?

A

Smaller ions with the same charge have higher charge densities so distort the carbonate ions more

39
Q

How can you test for Fe2+ ions?

A

Add OH- ions, a green ppt will form

40
Q

How can you test for Fe3+ ions?

A

Add OH- ions, a brown ppt will form

41
Q

What is the thermal decomposition of group 2 carbonates?

A

All group 2 carbonates undergo thermal decomposition to produce a metal oxide and carbon dioxide
The carbonate and metal oxide are both white solids, carbon dioxide is a colourless gas

42
Q

What is the solubility rule for group 2 carbonates?

A

Solubility decreases down the group, however none are very soluble

43
Q

What is the solubility rule for group 2 hydroxides?

A

Solubility increases down the group

44
Q

What hopes to first ionisation enthalpy down a group and across a period?

A

Down the group - First ionisation enthalpy decreases due to increasing atomic radius and electron shielding which reduce the effect of electrostatic forces of attraction

Along a period - First ionisation enthalpy increases due to decreasing atomic radius (from increasing nuclear charge) and greater electrostatic forces of attraction

45
Q

What does an emissions spectrum look like?

A

Bright lines on a dark background

46
Q

What does an absorption spectrum look like?

A

Dark lines on a coloured background

47
Q

What do both absorption and emission spectra have in common?

A

Both are line spectra
The lines are in the same position for any given element
Lines become closer at higher frequencies
Both a series of lines representing transitions to or from a particular energy level

48
Q

Lithium ion flame colour

A

Crimson red

49
Q

Sodium ion flame colour

A

Yellow

50
Q

Potassium ion flame colour

A

Lilac

51
Q

Calcium ion flame colour

A

Brick red

52
Q

Barium ion flame colour

A

Green

53
Q

Copper(II) ion flame colour

A

Blue-green

Chemistry Year 1 (5 decks)

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