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Chemistry > 1) Principles of chemistry - bonding > Flashcards

1) Principles of chemistry - bonding Flashcards

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
Properties of C60 fullerene
-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
Metallic bonding
Attraction between positive metal ions and negatively charged delocalised electrons -draw metallic lattice
27
Physical properties of metals
-high melting and boiling points -conduct electricity -malleable and ductile
28
Physical properties of metals - high melting and boiling points
-many strong metallic bonds in giant metallic structures -large amounts of heat energy needed to overcome forces and break bonds
29
Physical properties of metals - good conductors of electricity and heat
-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
Physical properties of metals - malleable and ductile
-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
Electrolytes
Ionic compounds that are: -in the molten state or -dissolved in water -ions are free to move
32
Electrolysis
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
Electrodes
-graphite rods -unreactive -can conduct electricity
34
Cathode
Negatively charged electrode -Positively charged ions move towards the cathode -gain electrons -reduction reactions always happen here
35
Anode
Positively charged electrode -negatively charged ions move towards the anode -lose electrons -oxidation reactions always happen here
36
Process of electrolysis - molten lead bromide
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
Electrolysis of aqueous solutions
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
Predicting products of electrolysis - cathode rules
-if metal is above hydrogen in the reactivity series, produce hydrogen gas -if metal is below hydrogen, form metal
39
Predicting products of electrolysis - anode rules
-if solutions of halides (chlorides, bromides, iodides), form the halogen -if solutions of any other common ions (sulfates, nitrates, hydroxides), form oxygen
40
Electrolysis of aqueous sodium chloride
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
Electrolysis of aqueous copper (II) sulfate
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
Electrolysis of dilute sulfuric acid
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
Practical: Investigate the Electrolysis of Aqueous Solutions
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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