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chemistry > chemical bonding > Flashcards

chemical bonding Flashcards

1
Q

How do many atoms react?

A

In order to achieve the electron configuration of a noble gas.

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2
Q

Ionic bonding

A

Electrons are transferred from metal to non-metal.
An electrostatic attraction between pos and neg ions.
Only conduct electricity when molten or aq. When electrons are transferred it creates ions and oppositely charged ions attract to form a giant ionic lattice.

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3
Q

What do square brackets in dot and cross diagram tell us?

A

Charge is spread over whole ion. The + and - ions are attracted to eachother by electrostatic forces of attraction.

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4
Q

Giant ionic lattice

A

Every ion in the lattice is attracted to every other oppositely charged ion.

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5
Q

Properties of ionic compounds

A
  1. High melting and boiling points as it takes a great deal of energy to overcome strong electrostatic forces of attraction
  2. Soluble in polar solvents
  3. Do not conduct electricity when solid
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6
Q

Covalent bonding

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
Between 2 non metals.
Electrons are shared.

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7
Q

How do scientists represent the 3D shapes of molecules?

A

Solid lines - these two bonds lie on the plane of the screen or page.

Solid wedge- this bond is coming out of the plane of the page.

Dotted wedge- this bond is projecting back behind the plane of the page.

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8
Q

What’s the electron pair repulsion theory?

A

The shape of a molecule is determined by the electron pairs surrounding the central atom as pairs of electrons repel all of the other electron pairs. The electron pairs move as far apart as possible to minimise repulsion.

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9
Q

Linear structure

A

2 electron pairs
180 degrees
straight line

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10
Q

trigonal planar

A

3 electron pairs
120 degrees

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11
Q

tetrahedral

A

4 electron pairs
109.5 degrees

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12
Q

trigonal bipyramidal

A

5 electron pairs
90- 120 degrees

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13
Q

octahedral

A

6 electron pairs
90 degrees

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14
Q

how do lone pairs repel?

A

more strongly then bonding pairs. this extra repulsion decreases other bond angles by 2.5 degrees.

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15
Q

pyramidal

A

3 bonding pairs and 1 lone pair
107 degrees

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16
Q

bent

A

2 bp and 2 lp
104.5 degrees

17
Q

nitrate ion

A

NO3-

18
Q

hydroxide ion

A

OH-

19
Q

ammonium ion

A

NH4-

20
Q

carbonate ion

A

CO3(2-)

21
Q

hydrogen carbonate ion

A

HCO3-

22
Q

sulphide ion

A

S2-

23
Q

sulphate ion

A

SO4 (2-)

24
Q

Charges in ionic compounds

A

Cancel out to produce an overall charge of 0

25
Q

What are isotopes?

A

Atoms of the same element with different numbers of neutrons and different masses.

26
Q

What is abundance?

A

Tells us how common each isotope is.

27
Q

How do we determine the mass no and abundance of isotopes?

A

Mass spectrometer

28
Q

What is relative isotopic mass?

A

The mass of an atom of an isotope compared with 1/12th the mass of carbon-12.

There is one relative isotopic mass for each isotope of an element.

It’s always a whole number.

Got no units.

29
Q

What is relative atomic mass?

A

The weighted mean mass of an atom of an element compared with 1/12th of an atom of carbon-12.

30
Q

How to calculate relative atomic mass?

A

Ar= ((relative atomic mass x % abundance of isotope 1) x (relative atomic mass x percentage adundance of isotope 2) ) divided by 100

31
Q

Simple covalent

A

Intermolecular forces. Shape determined by the no of electron pairs around the central atom and the repulsion between them. Each pair naturally repels each other so the largest bond angle possible exists between covalent bonds.

32
Q

Diamond

A

Carbon atoms each bonded to 4 further carbon atoms. Forms rigid tetrahedral structure making it one of the hardest materials known.

33
Q

Graphite

A

Each carbon atom is bonded to 3 others in flat hexagonal sheets which means there is one delocalised electron per carbon atom. These electrons can move freely allowing graphite to conduct electricity and can therefore be used in an electrode. The intermolecular forces between layers of graphite a weak and can slide over each other allowing it to be used as a lubricant.

34
Q

Metallic bonding

A

A giant lattice of positively charged ions surrounded by delocalised electrons. There are strong electrostatic forces of attraction between the oppositely charged part particles. Ions that are larger in size such as barium produce a weaker attraction due to their great atomic radius. Good conductors and delocalised electrons can carry a flow of charge. Also malleable as positive ions can slide over one another.
High melting points. Solid at room temperature.

chemistry (8 decks)

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