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Chemistry Salters B Aslevel > Elements of life > Flashcards

Elements of life Flashcards

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1
Q

What is the mass number?

A

The number of protons plus the number of neutrons

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2
Q

What is an isotope?

A

Atoms of the same element but with a different mass number because of having a different number of neutrons

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3
Q

What is Mass spectrometry?

A

The measure of the atomic mass of particles (atoms or molecules)

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4
Q

How does Mass spectrometry work?

A

Atoms or molecules are ionized and form cationos and are then separated based off mass and charge.

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5
Q

What is nuclear Fusion? and what must happen for it to occur?

A

When two lighter nuclei are combined to make a havier nucleus of a new element.
The nuclei must come very close to each other.

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6
Q

12-6-C. What do the two numbers represent?

A

The 12 is the mass.

6 is the number of protons (atomic mass)

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7
Q

What happens when electrons around an atom absorb light?

A

The electrons are raised from their ground state into an excited state.

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8
Q

What does the absorption spectrum look light and what does it signify?

A

It is a colored spectrum with black lines that signify what wavelengths of light have been absorbed by an atoms electrons.

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9
Q

What happens after and electron moves to its excited state?

A

It will fall back to its ground state which causes a photon to be released.

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10
Q

What does an emission spectrum look like? and what does it signify?

A

Black spectrum with colored lines that signify what frequency of light has been released.

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11
Q

What is Bohrs theory?

A

The theory of absorption and emission spectrum. It was the first indication of electrons. It also said that energy is quantised. Also linked the behavior of light as a particle and a wave

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12
Q

2 equations related to Bohrs theory:

A

Speed of light = Frequency x Wavelength

Energy of a photon = Plancks Constant x Frequency

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13
Q

What is the order of subshells? and how many electrons in each?

A

S (2 electrons), P (6 electrons), D (10 electrons) , F (14 electrons)

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14
Q

How do electron pairs orbit?

A

Opposite Directions

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15
Q

What is the shape of the S Subshell?

A

Spherical

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16
Q

What is the shape of the P Subshell?

A

Figure of 8

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17
Q

Describe how electrons fill sub shells:

A

They fill from the inside out and fill each pair of electrons evenly

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18
Q

Why do electron sub shells fill the way they do?

A

Because they fill up with the lowest energy configuration possible. Efficiency

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19
Q

Which part of the periodic table corresponds to S, P, D?

A

S: Group 1 and 2
P: Group 3 to 8
D: Transition Metals

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20
Q

How did Mendeleev arrange the periodic table? How is it arranged now?

A

Mendeleev: In order of relative atomic mass
Now: In order of number of protons

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21
Q

Describe covalent bonding?

A
  • Between two no-metalic atoms

- They share electrons

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22
Q

Describe a dative covalent bond?

A

A covalent bond but one electron donates more electrons than the other.

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23
Q

Describe the properties of a covalent bond.

A
  • Very strong bond so breaking it is very hard (requires more energy)
  • Electrostatic attraction between molecules is low so separating them is easily done (requires little energy)
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24
Q

How are molecular shapes formed?

A

Because regions of electron density are negatively charged and so repel each other. They move as far away as possible.

25
Q

Bond angle: Linear

A

180*

26
Q

Bond angle: Trigonal planar

A

120*

27
Q

Bond angle: Tetrahedral

A

109.5*

28
Q

Bond angle: Triganal bi pyramidal

A

120* and 90*

29
Q

Bond angle: Octahedral

A

90*

30
Q

What is a mole? and what is its value?

A

A quantity of something

6.02x10^23

31
Q

Equation for calculating the number of moles

A

Mass / Molar mass

32
Q

What is the empiracle formula?

A

The simplest molecular formula

33
Q

What is a molecular formula?

A

Condensed formula (atoms grouped together)

34
Q

Why might a yield be less than expected?

A
  • Loss of reactants
  • Side reactions
  • Impurities
  • Temperature or pressure change
  • Reaction not gone to completion
35
Q

How do you calculate your yield?

A

( Experimental yield / theoretical yield ) x 100

36
Q

What is water crystallization?

A

Water molecules are trapped in the molecule of crystal. This is a hydrated crystal

37
Q

How can water composition of a hydrated crystal be calculated?

A

Heating and evaporating the water and measuring the mass change.

38
Q

What does the equation for a hydrated crystal look like?

A

CuSO4 * 5H20

39
Q

What are the properties of S block elements?

A
  • Elements become more metallic as you go down the group
  • S block metals are weaker than other metals
  • They are all very reactive and so cannot be found pure
40
Q

What is first ionization enthalpy?

A

The energy required to remove and electron from the outer shell of an atom when it is in a gas state.

41
Q

What ion is formed when a gas is ionized during first ionization enthalpy?

A

Positive ion (cation)

42
Q

What is a Cation?

A

A positive ion

43
Q

What is an anion?

A

Negative ion

44
Q

What are the first ionization enthalpy trends?

A
  • The energy required increase as you move across the period because there are more protons holding the electrons in place
  • As you move down a group the energy required gets smaller because there are more shells and more electron shielding
45
Q

What is the equation for the first and second ionization reaction with calcium?

A

Ca ==> Ca+ + e-

Ca+ ==> Ca2+ + e-

46
Q

How do group 2 atoms react with oxygen?

A

They bond to make an oxide:

2M + O2 ==> 2MO

47
Q

How do group 2 atoms react with water? and what is produced?

A

They make hydrogen

M + 2H2O ==> M(OH)2 + H2

48
Q

What happens when you heat carbonates?

A

They form an oxide and Carbon dioxide

MCO3 ==> MO + CO2

49
Q

What are the properties of thermally decomposing group 2 carbonates? and why?

A
  • Harder to decompose down the group because the lower groups have a lower charge density and so form a more stable carbonate.
  • MgCO3 is less stable than CaCO3 so MgCO3 more readily breaks down
50
Q

How do group 2 oxides and hydroxides react with acids?

A

They form salts. e.g.
MO + HCl ==> MCl2 + H2O
M(OH)2 + H2SO4 ==> MSO4 + 2H2O

51
Q

Why are acids acidic?

A

Because they contain a H+ ion that dissociates in water

52
Q

Why are alkalis alkali?

A

Because they contain a OH- ion that dissociates in water.

53
Q

What happens when you combine a Acid and alkali? What is formed and how do they neutralise?

A

Acid + Alkali ==> Salt + Water

H+ + OH- ==> H20

54
Q

What is a base?

A

Any substance that accepts a H+ ion

55
Q

What happens when an acid and water combine? and what is formed?

A

The water accepts the H+ ion and forms an oxonium ion.
e.g.
HCl + H2O ==> H3O+ + Cl-

56
Q

What is the order for sub shells?

A

1s2 2S2 2P6 3S2 3P6 4S2 3D10 4P6 4D10 4F14

57
Q

What is the relative formula mass?

A

The sum of the Relative atomic masses of atoms in a molecule

58
Q

4 equations to make ionic salts?

A

Acid + Alkali ==> Salt + Water
Acid + Base ==> Salt + water
Acid + carbonate == > Salt + Water + Carbon dioxide
Acid + Metla ==> Salt + Hydrogen

59
Q

Describe metallic bonding?

A

Positive ions surrounded by a sea of delocalised electrons

Chemistry Salters B Aslevel (5 decks)

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