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Chemistry > Topic 1 & 3 > Flashcards

Topic 1 & 3 Flashcards

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1
Q

Nucleon number

Atomic number

A

N (mass):

  • num of protons and neutron
  • in the nucleus of one atom of an element

A (proton):

  • the number of protons
  • in the nucleus of one atom of an element
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2
Q

Proton Relative mass, relative charge
Neutron
Electron

A

Relative mass, relative charge

P 1, +1
N 1, 0
E 1/2000 (0.0005), -1

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3
Q

Isotope definition (2 m)

A
  • ATOMS with the same num of protons/atomic num

- but different num of neutrons/mass num

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4
Q

Relative Atomic mass

definition (3 m)

A

(Ar)

  • the avg mass of all the isotopes of an element
  • taking into account their percentage abundance,
  • relative to carbon-12
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5
Q

Calculating Ar

A

(mass num x % abundance) + … / 100

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6
Q

Period num & group num

A

period num = num of electron shells

group num = num of electrons on outer shell

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7
Q

Group 1

A

Alkali metals - they all react in a similar way as they all have 1 electron in their outer shell.

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8
Q

Group 2

A

Alkaline earth metals - react in a similar way:
2 electrons
in outer shell

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9
Q

Group 7

A

The Halogens - react in a similar way
7 electrons
in outer shell

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10
Q

Group 8/0

A

The Noble Gases
unreactive/ inert:
they have a full outer electron shell.

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11
Q

Properties of metals (6)

A
  • malleable(can change shape easily)
  • good conductors of heat and electricity (electrons are free to move)
  • sonorous (make a sound when hit)
    shiny
    ductile (stretch)
    high melting point - A lot of heat energy is needed to overcome forces and break strong metallic bonds in giant metallic structures
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12
Q

properties of non-metals (5)

A 
dull
brittle
poor conductors - fixed electrons
not sonorous
low melting point - weak intermolecular forces between the molecules
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13
Q

Ionic bonding

A

(metal + non-metal)

  • The electrostatic force of attraction between oppositely charged
  • ions
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14
Q

Describe, in terms of electrons, how an ionic bond in [sodium chloride] is formed. (3 m )

A
  • electron transfer
  • from sodium to chlorine
  • sodium has lost 1 electron (oxidised) and chlorine has gained 1 electron(reduced).
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15
Q

Relative Molecular Mass definition

A

(Mr)

sum of the relative atomic masses.

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16
Q

Element definition

A

Substance that cannot be broken down into anything simpler/

substance containing atoms with the same atomic number or proton number

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17
Q

Ionic bonding

structure & physical properties: conductivity and melting point

A

Structure: giant crystal lattice
(continuous ions) (regular, pattern of oppositely charged ions)

Properties:

  1. High melting point (solids at room temp)
    - requires large amount of energy to overcome
    - the STRONG
    - electrostatic forces of attraction between oppositely charged ions.
  2. Can conduct only when MOLTEN or in SOLUTION(dissolved)
    - ions
    - are free to move
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18
Q

Which has the highest melting point out of NaCl and MgO? (3 marks)

A
  • MgO has the higher melting point
  • greater charges of the Mg2+ ion and O2- ion relative the Na+ and Cl-
  • therefore stronger forces of attraction between ions in MgO
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19
Q

Covalent Bonding definition (2 m)

A

The electrostatic force of attraction between

  • a shared pair of electrons and
  • the positively charged nucleus of EACH ATOM
20
Q

Molecule definition (2 m)

A
  • a discrete number of atoms

- covalently bonded

21
Q

Properties of covalent molecules: structure, m & b points, conductivity

A

simple molecular structure (except diamond..etc)

(simple = discrete number of atoms
molecular = atoms covalently bonded)

Low m & b points:

  • weak
  • intermolecular forces of attraction
  • require little energy to overcome

Do NOT conduct - no charged particles that are free to move

22
Q

Solubility and Volatility of ionic and covalent compounds, monatomic, simple molecular, metallic

A

Volatility (A substance capable of readily changing from a solid or liquid form to a vapour)

All insoluble except ionic
Ionic - soluble, non-volatile (strong ionic bonds)
Covalent - insoluble, volatile
Monatomic - insoluble
Simple molecular - insoluble
Metallic - insoluble (reacts with water)
23
Q

Allotrope definition

A

different forms of the same element

24
Q

Diamond structure

A

C (s)

  • tetrahedral arrangement around each carbon
  • giant covalent structure
  • each carbon is covalently bonded to 4 others
25
Q

Diamond physical properties

A
  1. Extremely high melting, boiling points/ sublimation point:
    - giant covalent structure
    - many strong
    - covalent bonds
    - requires high amounts of energy to overcome
  2. Extremely strong: same
  3. Does not conduct electricity:
    - no free electrons
    - that can move
26
Q

Graphite structure

A
  • hexagonal layers of carbon atoms
  • giant covalent structure
  • layers can easily slide (due to weak forces of attraction between the layers)
  • each carbon is covalently bonded to 3 others
27
Q

Graphite physical properties

can act as what?, conductivity, melting/boiling point

A
  1. Soft/ Can act as a lubricant
    - layers can easily slide
    - due to the weak forces of attraction between the layers
  2. Good conductor of electricity
    - sea of delocalised electrons
    - that are FREE TO MOVE
    can be used in electrodes, brushes in electric motors
  3. Has a high m point/ sublimation point
    - giant covalent structure
    - many strong
    - covalent bonds
    - requires high amounts of energy to overcome
28
Q

Metallic bonding definition (2 marks)

A

the electrostatic forces of attraction between

  • the sea of delocalised electrons
  • and the fixed metal cations (+ve ion)
29
Q

Metallic bonding structure

A
  • giant metallic structure
  • cations are regularly arranged in layers
  • strong metallic bonds
30
Q

Metallic bonding physical properties

melting point, conductivity

A
  1. High melting point:
    - a lot of energy is required to overcome
    - the strong
    - metallic bonds
  2. Can conduct electricity & heat:
    - the sea of delocalised electrons are
    - FREE TO MOVE
  3. Malleable (able to change shape without breaking)
    - the layers of metal cations are regularly arranged
    - can easily slide
31
Q

What are alloys and why are they stronger than their corresponding metals?

A

mixture of 2 or more elements/compounds physically mixed.

  • the metal cations are irregularly arranged
  • so can no longer slide over each other
32
Q

Uses of mild steel [2] and stainless steel [2]

Name the uses of and stainless steel (chemical plant and cutlery)

A

Iron and Carbon

mild steel - car bodies and machinery - durable, strong and malleable

stainless steel (20% chromium & 10% nickel) - chemical plant and cutlery - strong and resistant to corrosion, hard

33
Q

Aluminium alloys uses (3)

A
  1. planes - low density to high strength ratio
  2. food containers - resistance to corrosion
  3. overhead cables - low density to high strength ration, good conductor, resistance to corrosion
34
Q

Silicon (IV) oxide

Structure, properties, conductivity

A

Structure

  • tetrahedral arrangement with one silicon atom and four oxygen atoms
  • each oxygen atom forms covalent bonds with 2 silicon atoms and
  • each silicon atom in turn forms covalent bonds with 4 oxygen atoms

same properties as a diamond

  1. Extremely high melting, boiling points/ sublimation point:
    - giant covalent structure
    - many strong
    - covalent bonds
    - requires high amounts of energy to overcome
  2. Extremely hard & strong: same
  3. Poor conductor/ Does not conduct electricity:
    - no free ELECTRONS
    - that can move
  4. insoluble
35
Q

a mole

A

1 mole of a substance contains 6.02 x 10^23 particles (Avogadro’s number)

36
Q

Empirical Formula definition

A

The smallest whole number ratio of atoms in a compound

37
Q

% yield

A

actual/ theoretical x 100

38
Q

% purity

A

pure yield/ total yield x 100

39
Q

give 2 major uses of sulfur dioxide (2)

A
  • Manufacture of sulfuric acid
  • bleach
  • making paper
    food/ fruit juice/ wine preservative
    fumigant/sterilising
40
Q

Brass consists of

A

zinc and copper

41
Q

state 2 uses of graphite which depend on the above properties

soft, good conductor of electricity

A

it is soft: pencils or lubricant or polish

good conductor: electrodes or brushes (in electric motors)

42
Q

why do sodium ions have a charge of +1? [1]

A

(they all have) 1 more proton than electrons / 11 protons and 10 electrons

43
Q

Aluminium is used to make food containers because it resists corrosion. Explain why is it not attacked by the acids in the food. [2]

A

protective/unreactive/resists/prevents corrosion/non-porous(layer) [1]
of (aluminium) oxide [1]

44
Q

3 uses of copper

A
  1. electrical wires - good conductor of electricity, malleable
  2. cooking utensils - low reactivity, good thermal conductivity
45
Q

uses of zinc 2

A

creates corrosion resistant, tough and conductive alloys = galvanising, making brass(Cu + Zn)

Chemistry (6 decks)

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