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Chemistry > Bonding+Structure > Flashcards

Bonding+Structure Flashcards

1
Q

What happens when metals form ions

A

They lose electrons from their outer shell to form a positive ion

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2
Q

What happens when non-metals form ions

A

They gain electrons from their outer shell to from a negative ion

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3
Q

Cation

A

Positive ion

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4
Q

Anion

A

Negative ion

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5
Q

What happens when a metal and non-metal react together

A

Metal loses electrons to form a positively charged ion and the non-metal gains these electrons to form a negatively charged ion

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6
Q

Force between an ionic bond

A

Electrostatic forces

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7
Q

What is an ionic bond

A

When a metal and non-metal react together

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8
Q

Negatives of a dot cross diagram

A
  • don’t show the structure of the compound
  • doesn’t show size of ions
  • doesn’t show how they’re arranged
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9
Q

What diagram is used to show an ionic bond

A

Dot cross diagram

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10
Q

Structure of an ionic compound

A

Giant ionic lattice

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11
Q

Formation of ionic lattice

A

-closely packed
-strong electrostatic forces of attraction between oppositely charged ions in all directions of lattice

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12
Q

Properties of ionic compounds

A

-high melting and boiling point due to strong bonds between ions. Takes a lot of energy to overcome attraction
-when solid, they can’t conduct electricity because the ions are held in place
-when ions melt, they’re free to move and they’ll carry electric charge
-some ionic compounds dissolve in water so ions separate and are all free to move in the solution so they’ll carry electric charge

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13
Q

What is a covalent bond

A

Where atoms share electrons with eachother so that they’ve got full outer shells

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14
Q

What elements use covalent bonding

A

Non-metal atoms and compounds

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15
Q

Displayed formula

A

Only lines (1 line=1 bond, 2 lines=2bonds)

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16
Q

Diagram for covalent bonds

A

Dot cross, over lapping lines, shared electrons

17
Q

What bonds are formed in simple molecular substances

A

Covalent

18
Q

Strength of simple molecular structures

A

-atoms held together with very strong covalent bonds
-intermolecular forces are very weak

19
Q

Properties of simple molecular structures

A

-low melting + boiling points (weak intermolecular forces)
-most molecular substances are gases or liquids at room temperature
-as molecules get bigger so do the intermolecular forces so more energy is needed to break them
-don’t conduct electricity, they just aren’t charged so no free electrons or ions

20
Q

Polymer

A

Lots of small units linked together to form a long molecule that has repeating sections.

21
Q

Bonds in a polymer

A

Covalent

22
Q

Intermolecular forces of polymers

A

-very large so more energy is needed to break them. Usually solid at room temperature
-still weaker than ionic or covalent bonds so they have lower melting and boiling points than ionic or giant molecular compounds

23
Q

Properties of giant covalent structures

A

-all atoms bonded to eachother by strong covalent bonds
-high melting a boiling points (lots of energy needed to break)
-don’t contain charged particles so they don’t conduct electricity not even when molten (except for graphite)

24
Q

Main examples of giant covalent structure

A

Diamond
Graphite
Silicon dioxide

25
Q

Silicon dioxide

A

-silica
-what sand is made of
-each grain of sand is one giant structure of silicon and oxygen

26
Q

What is an allotrope

A

Different structural forms of the same element in the same physical state

27
Q

Diamond

A

-giant covalent structure made up of carbon atoms
-each carbon atom has 4 covalent bonds which makes diamond really hard
-high melting point (string covalent bonds which need a lot if energy to break)
-doesn’t conduct electricity (no free electrons or ions)

28
Q

Graphite

A

-each carbon atoms forms 3 covalent bonds
-has one free delocalised electron: so it conducts electricity and thermal energy
-sheets of carbon atoms arranged in hexagons
-weak forces between layers so they can move over eachother freely
-this makes graphite soft and slippery: ideal lubricating material

29
Q

Graphene

A

-one layer of graphite
-one atom thick
-very light: can be added to composite materials to improve their strength without adding much weight
-also contains delocalised electrons so can conduct electricity through whole structure
-has the potential to be used in electronics

30
Q

What are fullerenes

A

Molecules of carbon, shaped like closed tubes or hollow balls

31
Q

Formation of fullerenes

A

-made up of carbon atoms formed in hexagons (or pentagons or heptagons)
-huge surface area- help make great industrial catalysts

32
Q

Uses of fullerenes

A

-can ‘cage’ other molecules, to deliver drugs into body
-can make great industrial catalysts
-can be good lubricants

33
Q

Nanotubes

A

-formed by fullerenes in cylinders
-can conduct electricity and thermal energy
-high tensile strength (don’t break when stretched)
-very high ratio between length and diameter

34
Q

Functions of nanotubes

A

-used in nanotechnology
-can be used in electronics or to strengthen materials without adding much weight such as tennis racket frames

35
Q

What happens in metallic bonding

A

-electrons of outer shell of metal atoms are delocalised
-strong forces of electrostatic attraction between positive metal ions and negative electrons
-these forces of attraction hold the atoms together in a regular structure known as metallic bonding. It’s very strong

36
Q

Properties of metals

A

-solid at room temp: strong electrostatic forces (high melt/boil points)
-good conductors of electricity and heat: delocalised electrons carry charge through whole structure
-malleable: layers of atoms can slide over eachother

37
Q

Alloys

A

-harder than pure metals
-mixture of 2 or more metals
-pure metals can be too soft
-when different atoms mix, the atoms are different sizes so it’s harder for them to slide over eachother, so they’re harder

Chemistry (11 decks)

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