Key Area 3: Bonding and Properties Flashcards

1
Q

Which is the most stable group?

A

Group 8 the noble gases

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2
Q

Chemical stability is achieved by?

A

Having a full outer shell

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3
Q

Three types of bonding?

A

Covalent (non-metal)
Ionic (metal + non-metal)
Metallic (metal)

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3
Q

Hydrogen and what are covalently bonded?

A

Non-metals in group 4,5,6,7

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3
Q

Covalent bonds

A

when positive nuclei from two atoms are held together by their common attraction for the shared pair of electrons

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3
Q

Molecular structure

A

H - H O=O etc.

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3
Q

Molecular formula

A

H2 O2 for diatomics

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4
Q

2 types of covalent structures

A

Covalent molecular
Covalent network

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5
Q

Polytomic molecules

A

Phosphorus P4
Sulfur S8

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6
Q

Hydrogen chloride

A

HCl, H - Cl, H - Cl, Linear

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7
Q

Water

A

H20, angular

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8
Q

Ammonia

A

NH3, Trigonal pyramidal

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9
Q

Methane

A

CH4 Tetrahedral

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10
Q

Covalent networks only appear in?

A

Solid states

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11
Q

Example of covalent network element?

A

Diamond

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12
Q

Properties of Diamond

A

Four unpaired electrons in outer shell
Very hard
Cannot conduct no free elctrons

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13
Q

Properties of Graphite

A

Only uses three of four electrons in outer shell
Soft slippery
Graphite can conduct bc theres a free electron

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14
Q

Example of covalent network compoud

A

Silicon dioxide

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15
Q

The structure is a network when its boiling point is?

16
Q

Atoms that lose electrons have?

A

More protons than electrons, have a positive charge

POSITIVE IONS

17
Q

Atoms that gain electrons have?

A

More electrons than protons, have a negative charge

NEGATIVE IONS

18
Q

Metal to have a full outer shell?

A

lose electrons

19
Q

Non-metals to have a full outer shell?

A

gain electrons

20
Q

Positive ions examples:

A

+ at top right

Litium atom = 2,1
Lithium ion = Li+

Magnesium ion = 2,8,2
Magnesium ion = Mg2+

(name stays the same)

21
Negative ion examples:
Chlorine atom = 2,8,7 Chloride ion = Cl- Oxygen atom = 2,6 Oxide ion = O-2 (name adds an -ide to the end)
22
Metal atoms become?
positive
23
Non-metal atoms become?
negative
24
2- SO 3 what does the three represent?
3 oxygen atoms present
25
2- SO 3 What does the 2- represent?
The charge
26
Ionic bonds form?
Ionic lattice
27
Two types of giant structures?
Covalent network Ionic lattice
28
Third compound structure?
Covalent molecular
29
If conducts as solid?
Metal
30
If low melting and high boiling point?
Covalent molecular
31
Ions not free to move in solid, conducts in liquid?
Ionic substance
32
High but never conducts?
Covalent network
33
Metal + non-metal =
Ionic
34
Non-metal + non-metal =
Covalent
35
If given non-metal + metal that is liquid at room temp?
Some sort of covalent bonding
36
Standard Solution
Is one whose concentration is known accuratley
37
weak forces of attraction are?
between molecules
38
strong forces of attraction are?
inside molecules
39
due to increasing strength....
between intermolecular forces
40
An ionic bond is?
the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.
41
A covalent molecular bond is?
when two positive nuclei are held together by their common attraction for a shared pair of electrons
42
Oxygen has?
Covalent bonds as diatomic