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Elements Of Life Flashcards

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1
Q

What is the atomic number

A

Protons and electrons

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2
Q

What is the mass number

A

Protons and neutrons

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3
Q

What is an isotope

A

Atoms of the same element with different neutron numbers

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4
Q

What is relative isotopic mass

A

Atoms isotopic mass compared with 1/12 of carbon-12 mass

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5
Q

What is relative atomic mass

A

Average mass of an atom of an element based on percentage abundancies of isotopes

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6
Q

What is relative formula mass

A

Mass of atom compared to another

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7
Q

What is relative molecular mass

A

Average mass of one molecule to 1/12 carbon-12 mass

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8
Q

When can’t relative molecular mass be used

A

If the bond is ionic

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9
Q

What is a mole

A

A substance amount containing 6.02x10^23 particles of substance

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10
Q

How is water crystallisation calculated

A 
Using a table
Mass
Mr
Moles
Ratio
And using the anhydrous mass of the element in the compound with water
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11
Q

What is molecular formula

A

Expression of number and type of atoms in a single substance

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12
Q

What is empirical formula

A

Simplest formula, ratio of elements in compound (once found moles of all divide all by the smallest mole)

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13
Q

How do you find the percentage composition of an element in a compound

A

Workout the relative formula mass of compound

Divide the elements Ar by the compounds Ar then x100

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14
Q

How do you find substance masses

A

Calculate the number of moles in the compound moles = conc x vol
Then calculate the mass using mass = mol x Mr

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15
Q

How do you do a titration calculation

A

Write the balanced symbol equation
Workout the moles of the neutraliser
Workout the moles of the element dissolved using the ratio and moles of the neutraliser
If need to scale up the volume e.g 25cm^3 to 1000cm^3 (25x40)=1000 so do the moles of the dissolved element x 40
Find the mass of the dissolved element
Workout the percentage purity actual(g)/all(g) x100

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16
Q

What is the percentage purity calculation

A

Actual (g) / all (g) x100

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17
Q

How do you make a standard solution

A

Workout number moles of solute needed
Workout number grams of solute needed (mass)
Weigh solute mass (first beaker then add mass)
Add small amount distilled wager to beaker dissolve solute then put in volumetric flask
Do rinsing did beaker and did
Too up flask to amount using pipette

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18
Q

How do you do a titration

A

Measure alkali into flask with indicator
Titration find neutralisation point
Do again accurate without indicator using same acid amount - titre

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19
Q

What is the equation to make a standard solution from a more concentrated one

A

Volume to use = final conc / initial conc x vol needed

Measure into volumetric flask top up with distilled water to needed volume

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20
Q

In s-sub shell how many orbitals are there and how many electrons does it hold

A

Has 1 s-orbital that holds 2 electrons

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21
Q

How many orbitals are there in the p-sub-shell and how many electrons can this hold

A

Had 3 p-orbitals that hold 6 electrons

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22
Q

In the d-sub-she’ll how many orbitals are there and how many electrons can it hold

A

Has 5 d-orbitals and can hold 10 electrons

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23
Q

In the f-sub-shell how many orbitals are there and how many electrons can it hold

A

There are 7 f-orbitals that can hold 14 electrons

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24
Q

Why are orbitals singly filled before pairing them

A

To keep the electrons as far apart as possible

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25
Q

How can you use the periodic table to find the outer sub-shell of an element

A

The block it is in e.g s is the last shell letter and the period that it is in is the small number

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26
Q

What were the Greeks contribution to discovering atoms

A

Matter made of invisible particles

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27
Q

What were the contributions John Dalton made to discovering atoms

A

Atoms are solid spheres make up different element

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28
Q

What were the contributions JJ Thomson made to discovering atoms

A

Plum pudding model, measured charge and mass

Discovered electrons

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29
Q

What were the contributions Rutherford made to discovering atoms

A

Saw alpha particles mainly not deflected by gold particles, mainly empty space with electron cloud
Later found that positive protons, different atoms have different protons

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30
Q

What were the contributions James Chadwick made to discovering atoms

A

Discovered neutrons

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31
Q

What were the contributions Bohr made to discovering atoms

A

If electrons in clouds, would spiral down, atom would collapse. Discovered shells, orbits that energy emitted/absorbed when electron move, fixed radiation frequency. Explained inert elements, why full shells are stable

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32
Q

Why is the 4s filled before the 3d sub shell

What are the exceptions

A

As it is closer to the nucleus
Copper - 3d^10 4s^1 is more stable to have full shell
Chromium - 3d^5 4s^1 is more stable half full shell, all orbitals have one electron, rather than fill 4s

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33
Q

What is nuclear fusion

A

Very high temperature, two light nuclei make heavier one. High pressure needed

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34
Q

What is covalent bonding

A

Non-metallic elements bond by sharing electrons. Atoms held together as positively charged nuclei attracted to negatively shared electrons

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35
Q

What is a dative covalent bond how is it drawn in a bond with the molecules

A

Contain lone pairs

When drawing the bonds the arrow points away from the atom donating the electron

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36
Q

What is an electron deficient molecule

A

AlCl3

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37
Q

How much does a lone pair ‘squash’ the structure by

A

2.5 degrees

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38
Q

What is simple molecular bonding, examples and what features does it have

A

Covalent molecular
Shared electron pairs. Weak intermolecular and strong covalent with non-metals e.g H2O, I2
Low melting/boiling point
No electrical conductivity
Insoluble in water (except oxygen, carbon dioxide, C2H5OH)
Soft

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39
Q

What is metallic bonding, examples and what features does it have

A

Giant lattice
Positive metal ions with a sea of delocalised electrons, force of attraction e.g Cu, Zn, K
High melting/boiling point expect mercury
Has electrical conductivity
Insoluble in water
Hard except for group 1 metals and mercury

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40
Q

What is ionic bonding, examples and what features does it have

A

Giant lattice
Positive and negative ions has electrostatic forces of attraction e.g NaCl, MgO
Metal and non metal except AlCl3, AlBr3, ACI3
High melting/boiling point
Has electrical conductivity when dissolved or molten (ions free)
Hard but brittle

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41
Q

What is giant covalent bonding, examples and what features does it have

A

Giant lattice
Two positive nuclei and two atoms attraction with same shared electrons e.g graphite, sand (SiO2), diamond
Non-metals
High melting/boiling point
No electrical conductivity except from graphite
Hardness high except graphite

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42
Q

What bond is it when there is 2 bonding pairs and no lone pairs and example

A

Linear
180 degrees
BeCl2

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43
Q

What bond is it when there is 3 bonding pairs and no lone pairs

A

Trigonal planar
120 degrees
AlCl3

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44
Q

What bond is it when there is 4 bonding pairs and no lone pairs

A

Tetrahedral
109.5 degrees
NH4, CH4

45
Q

What bond is it when there is 5 bonding pairs and no lone pairs

A

Trigonal bypyramid
90 degrees and 120 degrees
PF5, PCl5

46
Q

What bond is it when there is 6 bonding pairs and no lone pairs

A

Octahedral
90 degrees
SF5

47
Q

What bond is it when there is 3 bonding pairs and 1 lone pair

A

Pyramidal
107 degrees
NCl3, NH3

48
Q

What bond is it when there is 2 bonding pairs and 2 lone pairs

A

V-shaped or bent
104.5 degrees
H2S, H2O

49
Q

What line is used to show a bond in plane of paper

A

Full block line

50
Q

What line is used to show a bond behind paper plane

A

Dotted line

51
Q

What line is used to show a bond in front of paper plane

A

Block triangle

52
Q

What is a giant ionic lattice

A

Large repeating structure, minimises repulsion, maximises attraction

53
Q

What happens to melting/boiling point across period 3, what happens from silicon to phosphorus

A

Increase across period

Falls at silicon to phosphorus, as bonds between particles in phosphorus weaker, easier to overcome than silicon

54
Q

What happens across any period

A

Atomic radius decrease, nuclear charge/protons increase, no extra energy levels, no shielding

55
Q

What happens in period 2 and 3 and after 3 to the densities

A

Period 2 and 3 densities increase across period except gases rose to maximum in group 3 and then fall

56
Q

What happens after 92-uranium to the nuclear force between protons

A

Strong nuclear force holds protons together till around 92-uranium,overcome repulsion, all isotopes unstable

57
Q

What did Mendeleev do with the periodic table

A

Combined atomic mass ideas and reactivity, left gaps for elements
1886 germanium discovered proved it

58
Q

Which group is the alkali metals

A

Group 1

59
Q

Which group is the alkali earth metals

A

Group 2

60
Q

What happens down group 1 and 2 to the elements

A

More reactive down group as electrons further from nucleus due to more shielding

61
Q

Why are electrons harder to loose across the period

A

Less reactive across period, stringer nucleus electrons harder to loose

62
Q

What are the properties of metals

A

Shiny
Malleable
Conduct electrons and heat

63
Q

What are the properties of non-metals

A

Poor conductors of heat and electrons

64
Q

What is ionisation enthalpy

A

Energy to remove an electron from outermost atom shell. Always positive, as energy needed to break attraction
X(g) -> X^+ (g) + e^-

65
Q

What happens to the ionisation enthalpy across a period

A

Larger ionisation enthalpy as stronger nucleus, smaller atomic radius so harder to loose electron

66
Q

What happens between nitrogen and oxygen to cause the slight decrease as shared orbital

A

Electrostatic repulsion

67
Q

Why is there a lower first ionisation at boron

A

Fist electron removed from p sub-shell, higher in energy (further from nucleus)

68
Q

Why is there a lower first ionisation at oxygen

A

Electrons start to pair in orbitals, repel, less energy required to remove electron

69
Q

Why is the second ionisation higher

A

Fewer electrons but same protons so stronger attraction in second so need more energy to remove an electron
X^+(g) -> X^2+(g) + e^-

70
Q

What is formed when an S block oxide/hydroxide react with acid
What is it used for

A

Salt and water
MO/OH + acid -> salt + water
Has neutralising effect, used as fertilisers

71
Q

What are the properties of the S block

A

Soft

Low melting/boiling point

72
Q

What does group 2 metal and water form

A

Not usually on own group 2 metal react with water
2M + 2H2O -> 2M(OH)2 +H2
Water added to oxide to form hydroxide alkaline solution formed as group 2 are bases

73
Q

What is the equation when S block metal carbonate heated and what is this process

A

CaCO3 -> CaO +CO2

Thermal decomposition

74
Q

What happens to thermal stability down a group, how is it explained

A

Harder to decompose, thermal stability increases

Explained in charge density of cation charge concentration

75
Q

Does a smaller 2+ ion polarise a carbonate ion better, what effect does polarisation have on the ion when heated

A

Smaller 2+ ion, higher charge density can polarise negative charge cloud round carbonate ion, less stable, easily broken when heated

76
Q

What happens to group 2 hydroxide solubility down the group

A

Increases, for most group 2 compounds with -1 charge

77
Q

What happens to group 2 carbonate solubility down group

A

Decreases, for most group 2 metals compounds with -2 charge

78
Q

What is a base and what bases are there and what is a soluble base called

A

Substance accepts hydrogen ions
Proton acceptor
Metal oxide, metal hydroxide, metal carbonate
A soluble base - alkali

79
Q

What is the acid + metal reaction

A

Acid + metal -> salt + hydrogen

80
Q

What is acid + metal oxide reaction

A

Acid + metal oxide -> salt + water

81
Q

What is the acid + metal hydroxide reaction

A

Acid + metal hydroxide -> salt + water

82
Q

What is the acid + metal carbonate reaction

A

Acid + metal carbonate -> salt + carbon dioxide + water

83
Q

What is an acid

A

Substance that donates hydrogen ion H^+ in chemical reaction

Proton donors

84
Q

What is the Brönsted Lowry theory

A

Acids are proton donors, bases are proton acceptors

Hydrogen theory transfer

85
Q

What is the neutralisation ionic equation

A

Alkali reacts with acid, salt made - neutralisation reaction
H^+(aq) + OH^-(aq) -> H2O(l)

86
Q

What reactions with OH^- in ionic precipitation and what colour precipitates are formed

A

Cu^2+ +OH^- -> Cu(OH)2 blue
Fe^2+ +OH^- -> Fe(OH)2 green
Fe^3+ +OH^- -> Fe(OH)3 orange/brown

87
Q

What reactions with Ba^2+ in ionic precipitation and what colour precipitates are formed

A

SO4^2- +Ba^2+ -> BaSO4 white

88
Q

What reactions with Pb^2+ in ionic precipitation and what colour precipitates are formed

A

Pb^2+ +2I^- -> PbI2 bright yellow

89
Q

What reactions with AgNO3/Pb(NO3)2 in ionic precipitation and what colour precipitates are formed

A 
Halides
Cl^- + AgNO3 -> AgCl
Cl^- + Pb(NO3)2 -> PbCl white 
Br^- + AgNO3 -> AgBr
Br^- + Pb(NO3)2 -> PbBr cream
I^- + AgNO3 -> AgI
I^- + Pb(NO3)2 -> PbI yellow
90
Q

What test can you use to test which halide precipitate is formed

A

Mix with dilute NH3
Cl^- dissolves
Br^- partially soluble
I^- insoluble

91
Q

When are bases formed from group 2 oxides

A

When hydroxides added to water they form alkaline solutions

92
Q

What are the insoluble solids

A

Barium
Calcium
Lead
Silver sulfate

93
Q

In the electromagnetic spectrum when does frequency increase

A

From radiofrequency -> gamma rays

94
Q

In the electromagnetic spectrum when does wavelength increase

A

Gamma rays -> radiofrequency

95
Q

In the electromagnetic spectrum when does energy increase

A

Radiofrequency -> gamma rays

96
Q

What is the absorption spectra

A

Particles absorb some emitted radiation, light analysed from stars missing certain frequencies
Absorption lines are black, missing light frequencies absorbed by chromosphere particles

97
Q

What is the emission spectra

A

Atoms/molecules/ions in chromosphere absorb energy, raised from ground state - excited states. Lose extra energy, emit electromagnetic radiation, detecting emission spectra. Appear as coloured lines on black background

98
Q

What is the balmer series

A

Hydrogen emission spectrum (visible)

99
Q

What is the Lyman series

A

Hydrogen emission spectra (UV light)

100
Q

What is the atomic structure

A

Light from stars not continuous, has lines corresponding to absorption/emission of specific frequencies of light

101
Q

What does an energy level diagram show

A

Emission spectra

Larger energy gap deltaE the higher the frequency of electromagnetic radiation emitted

102
Q

What does E=hf workout

A

Photon light energy given off as electron falls

h - Planks constant - 6.63x10^-34?JHz(Js^-1)

103
Q

What is spectroscopy

A

Study how light, matter interact so can understand atoms electronic configuration

104
Q

What is the wave model of light

A

Wavelength, frequency behaviour
Wave of light travel distance certain time with speed, c = (3x10^8ms^-1)
Use c=wavelength x frequency

105
Q

What is the particle model of light

A

Light considered as stream of energy packets - photons. Energy of photons related to light position on electromagnetic spectrum

106
Q

What are the flame test and the colours

A 
Ion       Colour
Li^+     Bright red
Na^+   Yellow
K^+      Lilac
Ca^2+ Brick red
Ba^2+  Apple green
Cu^2+  Blue green
107
Q

How is the absorption and emission spectra linked

A

Energy/frequency of absorption black lines from 1->2 is the same as the emission coloured lines from 2->1

108
Q

How can mass spectra be used to calculate relative atomic mass of relative abundance

A

Each ion calculates from each peak height
Calculate RAM - relative isotopic mass x relative abundance / 100 + ..
No units as relative

109
Q

How can relative abundances be calculated

A 
E.g RAM of antimony = 121.8 
Has two isotopes, antimony-121 and -123
Ar = 121 x ?/100 + 123 x (100-?)/100   (x100)
12180 = 121? + 123(100-?)   (Expand)
12180 = 121? + 12300 - 123?    (Group)
123? - 121? = 12300 - 12180
2? = 120
? = 60
So antimony-121 = 60% and antimony-123 = 40%

Chemistry (5 decks)

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