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Chemistry > 1) Principles of chemistry - bonding > Flashcards

1) Principles of chemistry - bonding Flashcards

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1
Q

Ion

A

An electrically charged atom or group of atoms formed by the loss or gain of electrons
-in order to obtain a full outer shell of electrons

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2
Q

Anions

A

-negative ions
-form when atoms gain electrons
-more electrons than protons
-All non-metals gain electrons from other atoms to become negatively charged ions

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3
Q

Cations

A

-positive ions
-form when atoms lose electrons
-more protons than electrons
-All metals lose electrons to other atoms to become positively charged ions

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4
Q

Group 1,2,3 - metal ion charges

A

Group 1: 1+
Group 2: 2+
Group 3: 3+

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5
Q

Transition metal charges - silver, copper, iron(II), iron(III), lead, zinc

A

Silver: Ag+
Copper: Cu2+
Iron (II): Fe2+
Iron (III): Fe3+
Lead: Pb2+
Zinc: Zn2+

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6
Q

Compound ion charges - hydroxide, ammonium, carbonate, nitrate, sulfate, ethanoate

A

Hydroxide: OH-
Ammonium: NH4+
Carbonate: Co3 2-
Nitrate: NO3-
Sulfate: SO4 2-
Ethanoate: CH3COO-

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7
Q

Group 5,6,7 non metal ion charges

A

Group 5: 3-
Group 6: 2-
Group 7: 1-

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8
Q

Ionic bonding

A

Strong electrostatic forces of attraction between oppositely charged ions

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9
Q

Giant ionic lattices

A

-ionic compounds are made of charged particles called ions which form a giant lattice structure

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10
Q

Ionic compounds characteristics

A

-high melting and boiling point - due to presence of strong electrostatic forces acting between oppositely charged ions
-forces act in all directions and a lot of energy is required to overcome them
-usually solid at room temperature
-non volatile
-usually water soluble

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11
Q

Ionic compounds - conductivity

A

-Can conduct electricity in molten/ solution - as they have ions that can move and carry charge
-Cannot conduct electricity in the solid state - ions are in fixed positions within the lattice and are unable to move

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12
Q

Covalent bonding

A

The electrostatic attraction between positive bonding nuclei and shared pair of bonding electrons

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13
Q

Simple covalent molecules characteristics

A

-weak intermolecular forces between individual molecules
-do not conduct electricity - do not contain free electrons - insulators

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14
Q

Covalent bonding - diatomic molecules: hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride

A

Hydrogen: H-H
Chlorine: Cl-Cl
Oxygen: O=O
Nitrogen: N≡N
Hydrogen chloride: H-Cl

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15
Q

Covalent bonding - inorganic molecules: water, ammonia, carbon dioxide

A

Water: H-O-H
Ammonia: H-N-H (another H from the bottom of N)
Carbon dioxide: O=C=O

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16
Q

Covalent bonding - organic molecules: methane, ethane, ethene

A

Methane: 4 H branching from 1 C
Ethane: C-C and 3 H branching off each C
Ethene: C=C and 2 H branching off each C

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17
Q

Simple molecular structures

A

have covalent bonds joining the atoms together
-intermolecular forces that act between neighbouring molecules
-low melting/ boiling points - weak intermolecular forces
-most molecules are either gases or liquids at room temperature - if are weak compared to covalent bonds
-liquids are volatile

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18
Q

When simple molecular structures increase in size

A

-the intermolecular forces also increase as there are more electrons available
-causes the melting and boiling points to increase

19
Q

Giant covalent structures

A

-have a huge number of non-metal atoms bonded to other non-metal atoms via strong covalent bonds
-giant lattices
-high melting and boiling points
-diamond, graphite, silicon dioxide

20
Q

Structure of diamond

A

-allotrope of carbon
-each carbon atom bonds with four other carbons - tetrahedron
-all covalent bonds are identical
-very strong
-no intermolecular forces

21
Q

Properties of diamond

A

-does not conduct electricity - no freely moving charged particles to the current
-very high melting point - four covalent bonds are very strong, extend in a giant lattice
-very hard

22
Q

Graphite

A

-each carbon atom in graphite is bonded to three others
-form layers of hexagons
-leave one free electron per carbon atom
-free electrons are free to move and carry charge - can conduct electricity
-covalent bonds within the layers are very strong, but the layers are attracted to each other by weak intermolecular forces
-layers can slide over each other
-makes graphite soft and slippery

23
Q

Properties of graphite

A

-conducts electricity and heat
-high melting point
-soft and slippery

24
Q

C60 fullerene

A

-60 carbon atoms are joined together forming 20 hexagons and 12 pentagons which produce a hollow sphere
-not giant, is a simple molecular structure

25
Q

Properties of C60 fullerene

A

-soft, low melting point -weak intermolecular forces between atoms which takes little energy to overcome
-cannot conduct electricity - even though there are delocalised electrons, they cannot jump between different molecules

26
Q

Metallic bonding

A

Attraction between positive metal ions and negatively charged delocalised electrons
-draw metallic lattice

27
Q

Physical properties of metals

A

-high melting and boiling points
-conduct electricity
-malleable and ductile

28
Q

Physical properties of metals - high melting and boiling points

A

-many strong metallic bonds in giant metallic structures
-large amounts of heat energy needed to overcome forces and break bonds

29
Q

Physical properties of metals - good conductors of electricity and heat

A

-free electrons that can move and carry charge
-electrons entering one end of metal cause delocalized electron to displace itself from the other end

30
Q

Physical properties of metals - malleable and ductile

A

-layers of positive ions can slide over one another
-metallic bonding not disrupted as valence electrons do not belong to any particular metal atom and can move with layers of positive ions
-metallic bonds not broken, strong and flexible

31
Q

Electrolytes

A

Ionic compounds that are:
-in the molten state
or
-dissolved in water

-ions are free to move

32
Q

Electrolysis

A

Process which electrical current from a dc supply breaks down electrolytes
-free moving ions in electrolytes are attracted to the oppositely charged electrodes which are connected to the dc supply

33
Q

Electrodes

A

-graphite rods
-unreactive
-can conduct electricity

34
Q

Cathode

A

Negatively charged electrode
-Positively charged ions move towards the cathode
-gain electrons
-reduction reactions always happen here

35
Q

Anode

A

Positively charged electrode
-negatively charged ions move towards the anode
-lose electrons
-oxidation reactions always happen here

36
Q

Process of electrolysis - molten lead bromide

A

Pb2+ ions gain electrons at the cathode
-become Pb atoms
Pb2+ + 2e- –> Pb
Br- ions lose electrons at the anode
-become Br atoms, pair up to form Br2 molecules (diatomic)
2Br- –> Br2 + 2e-

-grey lead metal forms at the negative electrode - deposits at the bottom of electrode
-brown bromine gas forms at the positive electrode (anode) - bubbling

37
Q

Electrolysis of aqueous solutions

A

Water is a weak electrolyte
-when electricity passes through
-ionises slightly, forming H+ and OH-
Therefore during electrolysis, there are four ions completing:
-anion and cation from ionic substance
-H+ and OH- from water

38
Q

Predicting products of electrolysis - cathode rules

A

-if metal is above hydrogen in the reactivity series, produce hydrogen gas
-if metal is below hydrogen, form metal

39
Q

Predicting products of electrolysis - anode rules

A

-if solutions of halides (chlorides, bromides, iodides), form the halogen
-if solutions of any other common ions (sulfates, nitrates, hydroxides), form oxygen

40
Q

Electrolysis of aqueous sodium chloride

A

Cathode:
Sodium above hydrogen
Hydrogen forms H2 molecules
2H+ + 2e- –> H2
-pop with lit split

Anode:
Attracts Cl-/ OH- ions
Cl- more reactive
Forms Cl2 molecules
2Cl- –> Cl2 + 2e-
-bleaches litmus paper

Remaining solution: Na+/ OH- left over, form a solution:
Sodium hydroxide solution - alkaline

41
Q

Electrolysis of aqueous copper (II) sulfate

A

Cathode:
Cooper below hydrogen
Form copper atoms
Cu2+ + 2e- –> Cu
-pink brown deposit seen

Anode:
SO4 2- not a halide, so oxygen forms
4OH- –> 2H2O + O2 + 4e-
-relights glowing splint

Remaining solution: H+/ SO4 2-
Forms H2SO4 - sulfuric acid

42
Q

Electrolysis of dilute sulfuric acid

A

Cathode:
Only have H+ ions
2H+ + 2e- –> H2
-pop with lit splint

Anode:
SO4 2- not halide, oxygen forms
4OH- –> 2H2O + O2 + 4e-
Twice as much H2 is formed compared to O2
-relights glowing splint

43
Q

Practical: Investigate the Electrolysis of Aqueous Solutions

A
  1. Add the aqueous solution to a beaker, cover the electrodes with solution
  2. Invert two small test tubes onto electrodes
  3. Connect the electrodes to a power pack or battery, turn on
  4. Observations at each electrode are made
  5. Gases collected in the test tube can be tested and identified

Chemistry (6 decks)

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