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Chemistry > Elements of Life > Flashcards

Elements of Life Flashcards

1
Q

Hydrochloric Acid

A

HCl

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2
Q

Nitric Acid

A

HNO3

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3
Q

Sulphuric Acid

A

H2SO4

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4
Q

Phosphoric Acid

A

H3PO4

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5
Q

Methanoic Acid

A

HCOOH

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6
Q

Ammonia

A

NH3

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7
Q

Isotopes

A

Different atomic number same mass number
Different number of neutrons same number of protons

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8
Q

Relative Atomic Mass

A

A measure of the average mass of an element compared to a standard unit of mass

Calculated by adding all masses of an element then averaging them based on their abundance

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9
Q

Atomic Mass

A

The actual mass of an individual isotopes - a fixed value

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10
Q

How to calculate RAM

A

Need abundance of each isotope
Need the mass number
(mass * abundance) + (mass * abundance)/(abundance + abundance)

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11
Q

Example of RAM with Chlorine

A

Cl-35 75%
Cl-37 25%

(75 * 35) + (37 * 25)/ 75 + 25 = 35.5

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11
Q

Atom

A

The smallest piece of an element, made up of protons, neutrons and electrons and has a neutral charge

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12
Q

Molecule

A

A group of atoms held together by covalent bonds

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13
Q

Ion

A

An atom or molecule which has lost or gained electrons so is positively or negatively charged

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14
Q

Element

A

A substance made from one type of atom only

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15
Q

Compound

A

A substance formed from two or more chemically bonded elements in a fixed ratio, shown by a chemical formula

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16
Q

Simple Structure

A

Made up of small molecules held together by weak intermolecular forces

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17
Q

Giant lattice structure

A

A 3-dimensional structure of particles held together by strong bonds (covalent or metallic)

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18
Q

Group

A

A vertical column in the periodic table. The element has the same number of outer electrons hence similar chemical properties

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19
Q

Intermolecular Forces

A

Attractive forces between neighbouring molecules

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20
Q

Neutralisation Reactions

A

Acid + Base –> Salt + Water

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21
Q

Combustion

A

Complete - +O2 —> CO2 + H2O
Incomplete - +O2 —> CO + H2O

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22
Q

Acid + Metal Carbonate

A

—> Salt + Water + Carbon Dioxide

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23
Q

Acid + Metal Oxide

A

—> Salt + Water

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23
Q

Acid + Metal Hydroxide

A

—> Salt + Hydrogen + Water

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24
Q

Common Acids

A

H+ Donors
Hydrochloric - HCl
Nitric - HNO3
Sulfuric - H2SO4
Phosphoric - H3PO4

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24
Q

Acid + Metal

A

—> Salt + Hydrogen

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24
Q

Common Alkalis/Bases

A

H+ Acceptors
Group 1 hydroxides + Oxides = Na2O
Group 2 hydroxides + Oxides = MgO

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25
Q

Polyatomic Ions

A

Hydrogen Sulfate - HSO4-
Carbonate - CO3 2-
Ethanoate - CH3COO-
Hydroxide - OH-
Sulphate - SO4 2-
Nitrate - NO3-
Hydrogen Carbonate - HCO3-
Ammonium - NH4+

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26
Q

Ar

A

Relative Atomic mass (average mass of an atom)

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27
Q

A

A

Atomic Mass (number of P+ and e-)

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28
Q

Z

A

Atomic Number (number of p+)

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29
Q

Nucleons

A

Protons and neutrons as they’re found in the nucleus

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30
Q

Avogadro’s constant

A

6.022 * 10^23

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31
Q

Molecular Formula (Mr)

A

Shows the actual number of atoms of each element present in a compound or molecule
Glucose’s Mr = C6H12O6

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32
Q

Empirical Formula

A

The simplest whole ratio of atoms of each element
Glucose = CH2O

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33
Q

Water of Crystallisation

A

Water that’s trapped between ions when an ionic solid forms
Ionic solids with woc = hydrated
Ionic solids without woc = anhydrous

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34
Q

woc shown in a formula

A

.xH2O where x = a number

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35
Q

Simple experiment for woc

A

1) Weigh crucible before and after hydrated solid is added
2) Place above bunsen burner
3) Stop heating, cool it, weigh it
4) Repeat until constant mass

36
Q

Nuclear Fusion

A

2 small nuclei join to make a larger nucleus
Only occurs at a high temp and high pressure - lots of energy needed to overcome repulsion between 2 positive nuclei

37
Q

Nuclear Fusion equations

A

add top numbers together and bottom numbers
12C + 4 He —> 16 BE
6 2 8

38
Q

Solute

A

The solid in the solution

39
Q

Solvent

A

The liquid that the solute is getting dissolved in

40
Q

1dm^3 in litres

A

1 litre

41
Q

Concentration equation

A

Conc=mol/volume (volume = dm3 (cm3/1000))

42
Q

Titration use

A

Used to find the concentration of one solution

43
Q

Volumetric Pipette

A

Rinse with what it’s measuring
Touch tip to the surface when emptying
Normally 25cm3

44
Q

Burette

A

Rinse with what it’s measuring
Read to 2d.p - last digit = 5 or 0
Bottom of meniscus

45
Q

Method of titration calculations

A

1) Write a balanced equation
2) Write information underneath (average titre or 25cm3)
3) Calculate the moles = conc * dm3
4) Use Stoichiometric ratio to determine moles of other reactant
5) Calculate conc (mol/dm3) give to 3s.f

46
Q

Acid

A

H+ donor

47
Q

Base

A

H+ receiver

48
Q

gcm-3

A

Convert to moles then times by 1000 - mass/mr * 1000

49
Q

gmdm-3

A

Convert to moles - mass/mr

50
Q

v/v

A

Find percentage then times by 1%

51
Q

PPM

A

Parts per million
ppm/1000 = dm3
Then moles = mass/mr

52
Q

Ionic Compounds

A

Giant lattices
Regular structure
Ions of opposite charge in a fixed ratio

53
Q

Ionic Compounds definition

A

The electrostatic attraction between oppositely charged ions
No e- transfer
Not always metal and non-metal

54
Q

Proof of ionic compound

A

Presence of a polyatomic ion
One from LHS and one from RHS

55
Q

Ionic compound conductivity

A

Conduct when molten
Conduct if dissolved
No conduction if solid
-Ions are free to move around when not solid

56
Q

Ionic Compound Mpt/Bpt

A

High due to electrostatic forces requiring energy to overcome
Also has a giant lattice that requires lots of energy to overcome

57
Q

Ionic Compound Solubility

A

Many dissolve in water
Water molecules interact with salts surface ions.
If soluble, the H+ attracts the anion and the O2- attracts the cation.

Ions that are pulled away are called hydrated ions
Held in place by ion-dipole forces

58
Q

Ionic dot and cross

A

Coefficient [M] charge Coefficient[NM]charge

59
Q

Standard Solution

A

We know the concentration very accurately

60
Q

s orbitals

A

Spherical, one on each energy level

61
Q

p oribtals

A

Dumbell shaped, 3 on each energy level except n = 1

62
Q

d orbitals

A

Crazy shapes, 5 on each energy level starting at n = 3

63
Q

f oribtals

A

Crazy hapes, 7 on each energy level starting at n = 5

64
Q

D block when writing

A

Always lags one behind

65
Q

Rule of noble gases in configuration

A

Use noble gas before and add remaining letters

66
Q

Ionisation energy

A

The energy required to remove the outermost electron from 1 mole of gaseous atoms

67
Q

Ionisation energy equations

A

Mg(g) –> Mg+(g) + e-
Cl (g) –> Cl+(g) + e-

68
Q

Successive ionisation energy

A

Electrons are removed one after the other from the same atom
e.g
1) Cl(g) –> Cl+(g) + e-
2) Cl+(g) –> Cl2+ (g) + 2e-

69
Q

Ionisation energy trend

A

Each time, more is required as same number of protons is attracting fewer electrons

70
Q

Absorption Spectra

A

Black lines
Rainbow background
When electrons move from a low EL to a high EL

71
Q

Emission Spectra

A

Coloured lines
Black Background
When electrons move from a high El to a low EL

72
Q

Spectra line spacing

A

Lines are always closer on the high frequency end of the scale (purple)

73
Q

Absorption and Emission lines same element

A

Same elements will have the spectra lines in the same place as the ELs are the same so the frequency released matches the frequency absorbed

74
Q

Absorption and Emission lines different element

A

Different elements have different spectra lines as the gaps between the ELs are different

75
Q

Model Answer for for spectrum

A

Only some frequencies of light are emitted or absorbed for a particular element as the energy levels are fixed (quartised) and the electrons can only move between energy levels

76
Q

Frequency equation

A

change in energy = plancks constant * frequency

77
Q

Wavelength calculation

A

speed of light = wavelength * frequency

78
Q

wavelength value

A

nanometres (*10^-9)

79
Q

Metallic bonding definition

A

The electrostatic attraction between a lattice of positive metal ions and a sea of delocalised electrons

80
Q

Metallic structure

A

-Giant
-Delocalised electrons (constantly moving)
-Charge written inside the circles (+, 2+ etc..)
-As positive charge increases, size of ions decrease

81
Q

Metallic Bonding Mpt/Bpt

A

Very high due to giant structure
Very high due to strong attraction between ions and delocalised electrons

82
Q

Metallic Bonding Conductivity

A

Very conductive due to delocalised electrons being free to move

83
Q

Metallic Bonding Solubility

A

Insoluble in H2O, forces of attraction between ions and e- are very strong

84
Q

Covalent Bonding Definition

A

The electrostatic Attraction between shared pairs of electrons and two positive nuclei

85
Q

Covalent Structures

A

Can be simple or giant. Simple is much more common than giant

86
Q

Examples of giant covalent structures

A

Diamond
Graphite
Silicon dioxide

87
Q

Covalent bonding trends

A

No of pairs increases
Type of bond increases (single, double and triple)
Relative bond length decreases
Relative bond strength increases

Two double bonds next to each other are not possible

88
Q

Explanation of dative bond

A

Electrons are shared so in most cases the atoms have a complete outer energy level. Most bonds have an electron from each atom but in some covalent bonds, both electrons come from one atom (a dative bond)

89
Q

Covalent bonding rules

A

No of covalent bonds normally = 8 - group number
e.g C = 8 - 4 = 4
H only makes 1 bond
Be makes 2 bonds due to 2 outer electrons
Al makes 3 bonds due to 3 outer electrons
P makes 8 - 5 =3 bonds or 5 bonds due to outer electrons
S makes 8 - 6 = 2 bonds of 6 bonds due to outer electrons

90
Q

Dot and Cross diagram

A

1) Check it’s covalent (RHS + Beryllium)
2) Draw the molecule with lines and check all atoms have the correct number of bonds
3) Replace each lines with a dot or a cross
4) Add lone pairs (group number - e- used for bonding)

91
Q

Dative bonds

A

A covalent bond where one atom donates both e-
Shown by an arrow

Chemistry (8 decks)

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