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Year 11 Additional Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Mass number =

A

Top number

Total number of protons and neutrons

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2
Q

Atomic number

A

Bottom number

Number of protons

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3
Q

How are compounds formed

A

Two or more elements chemically joined together

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4
Q

What are isotapes

A

Different atomic forms of the same element, which have the SAME number of PROTONS but DIFFERENT number of NEUTRONS

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5
Q

Ionic bonding

A

Atoms LOSE or GAIN electrons to form CHARGED particles (called ions)

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6
Q

Ionic compounds

A
  • Have regular ionic lattices
  • Form a closely packed regular lattice arrangement
  • Similar properties
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7
Q

Ionic compounds properties

A
  • high melting & boiling points (strong attraction)
  • melt -> free to move
  • carry electrical current
  • dissolve easily
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8
Q

Which groups are most likely to form ions

A

Groups
1 & 2
6 & 7

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9
Q

Ions have the electronic structure of a

A

Noble gas

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10
Q

What happens to group 1 and 2 elements

A

They lose electrons to form positive ions

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11
Q

What happened to group 6 and 7

A

The gain elections to form negative ions

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12
Q

What forms an ionic compound

A

Positive ions combine with negative ions to form ionic compounds

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13
Q

Wha is the overall charge of any compound

A

Zero

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14
Q

The negative charges ——- the positive charges

A

Balance

E.g. Na+ and Cl- = +1 + -1 = 0 The charges are balanced to for NaCl

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15
Q

What is covalent bonding

A

Sharing electrons with other atoms

Both atoms have a full outer shell

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16
Q

Substances with covalent bonds can either be —–

A

Simple molecules or giant structures

17
Q

Explain a simple molecular structure

A
  • Atoms have strong bonds
  • Forces of attraction are weak
  • Melting & boiling points are low (easily parted)
  • Don’t conduct electricity
  • No ions or electrical charge
18
Q

Giant covalent structures are

A

Macromolecules

19
Q

Giant covalent structures

A
  • Atoms are bonded by strong covalent bonds
  • High melting and boiling points
  • Don’t conduct electricity
  • Example - diamond
20
Q

Metallic structures

A
  • Consists of giant structures
  • Have free electrons -> good heat and electricity conductors
  • Allow layers to slide over each other/bent/shaped
21
Q

Alloys are harder than

A

Pure metals

22
Q

Pure metals

A
  • Have different sized atoms
  • Distort the layers
  • More difficult for layers to slide over each other
23
Q

Draw the ionic structure of Sodium Chloride

A

Na+ Cl-

24
Q

Draw the ionic structure of calcium oxide

A

Cl- Ca2+ Cl-

25
Q

Draw the covalent bond of Hydrogen and Chlorine

A

H-H Cl-Cl

26
Q

Simple molecules definition

A

A few atoms held together by strong covalent bonds.

An example is carbon dioxide (CO2), the molecules of which contain one atom of carbon bonded with two atoms of oxygen.

27
Q

Properties of simple molecular substances

Low melting and boiling points

A

This is because the weak intermolecular forces break down easily.

28
Q

Properties of simple molecular substances

Non-conductive

A

they do not have any free electrons or an overall electric charge.

29
Q

Giant covalent structures definition

A
  • Contain a lot of NON- METAL ATOMS joined to adjacent atoms by covalent bonds.
  • Atoms are arranged into giant regular lattices - extremely STRONG STRUCTURES because of the many bonds involved.
30
Q

Properties of giant covalent structures

Very high melting points

A

a lot of strong covalent bonds must be broken. Graphite, for example, has a melting point of more than 3,600ºC.

31
Q

Properties of giant covalent structures

Variable conductivity

A

Diamond does not conduct electricity. Graphite contains FREE ELECTRONS , so it DOESN’T conduct electricity. Silicon is semi-conductive - that is, midway between non-conductive and conductive.

32
Q

Metals have a

A

Giant structure

33
Q

Why do metallic bonds have free electrons

A

Produce all the properties of metals

34
Q

Where do free electrons come from

A

The outer shell of every atom in the structure

35
Q

Metals are

A

good conductors of HEAT and ELECTRICITY

36
Q

How do electrons hold atoms together

A

They have strong forces of electrostatic attraction between positive metal ions and negative electrons

Year 11 Additional Chemistry (5 decks)

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