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Chemistry Topic 2 > 2.2.2- Bonding And Structure > Flashcards

2.2.2- Bonding And Structure Flashcards

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1
Q

What is an ionic bond?

A

The electrostatic force of attraction between oppositely charged ions formed by electron transfer

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2
Q

What properties do ionic structures have?

A

-high melting points due to strong electrostatic forces
-conduct electricity when molten or dissolved as ions are mobile
-usually soluble
-brittle

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3
Q

When is ionic bonding strongest?

A

When ions are smaller and/or have different charges

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4
Q

What is a metallic bond?

A

Attractions between positive metal ions and delocalised electrons

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5
Q

What are the properties of metallic structures?

A

-high mp due to strong electrostatic attraction
-conduct electricity

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6
Q

What is a covalent bond?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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7
Q

What properties do covalently bonded molecules have?

A

-low mp due to weak IMFs
-don’t conduct electricity

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8
Q

What covalent bonds are the strongest?

A

Shorter bonds as the atoms are held closer together

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9
Q

What bonds are shortest?

A

Double and triple bonds

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10
Q

What is average bond enthalpy?

A

A measurement of covalent bond strength

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11
Q

What is a dative covalent bond?

A

Formed when both of the electrons in the shared pair come from one of the bonding atoms

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12
Q

How is a dative covalent bond indicated?

A

By an arrow from the lone electron paid

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13
Q

What is the Valence Shell Electron Pair Repulsion Theory (VSEPR)?

A

Simple covalent molecules have a 3D shape due to repulsion

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14
Q

How do electrons repel eachother?

A

Equally

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15
Q

What does a solid line indicate?

A

A bond that is in the plane of the paper

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16
Q

What does a wedged line indicate?

A

A bond that comes out of the plane of the paper

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17
Q

What does a dotted line indicate?

A

A bond that goes into the plane of the paper

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18
Q

How do lone pairs repel?

A

They repel more than bonding atoms, reducing the bonding angle by 2.5° per lone pair

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19
Q

How many bonding and lone pairs does a linear shape have?

A

2 bonding, 0 lone

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20
Q

What bond angle does a linear shape have?

A

180°

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21
Q

How many bonding and lone pairs does a trigonal planar shape have?

A

3 bonding, 0 lone

22
Q

What is the bond angle of a trigonal planar shape?

A

120°

23
Q

How many bonding and lone pairs does a tetrahedral shape have?

A

4 bonded 0 lone

24
Q

What bond angle does a tetrahedral shape have?

A

109.5°

25
Q

How many bonding and lone pairs does a trigonal pyramidal shape have?

A

3 bonded 1 lone

26
Q

What bond angle does a trigonal pyramidal shape have?

A

107°

27
Q

How many bonding and lone pairs does a bent shape have?

A

2 bonded 2 lone

28
Q

What is the bond angle of a bent shape?

A

104.5°

29
Q

How many bonding and lone pairs does an octahedral shape have?

A

6 bonded 0 lone

30
Q

What is the bond angle of an octahedral shape?

A

90°

31
Q

How many bonding and lone pairs does a trigonal bipyramidal have?

A

5 bonded 0 lone

32
Q

What bond angles does a trigonal bipyramidal shape have?

A

90° and 120°

33
Q

What is electronegativity?

A

The relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself

34
Q

What are the most electronegative atoms?

A

Fluorine, Oxygen, Nitrogen, and Chlorine

35
Q

What is the trend of electronegativity?

A

-Increases along a period
-decreases down a group

36
Q

Why does electronegativity increase when going along a period?

A

Number of protons increase which decreases atomic radius as electrons are pulled in more

37
Q

Why does electronegativity decrease as you go down a group?

A

Shielding increases which increases the atomic radius as the shells are further away from the nucleus

38
Q

How can you compare the electronegativity of atoms?

A

Using the Pauling scale

39
Q

What is non polar?

A

The bonded electron pair is shared equally between the bonded atoms

40
Q

When is an atom non polar?

A

When the bonding atoms are the same, or they have similar electronegativities

41
Q

What is polar?

A

The bonded electron pair is shared unequally

42
Q

When is an atom polar?

A

When the bonding atoms have different electronegativity values

43
Q

What does a polar molecule cause?

A

Produces a charge separation called a dipole

44
Q

Why do some non polar molecules have polar bonds?

A

The dipoles can cancel out due to direction

45
Q

What is an intermolecular force?

A

Weak interactions between dipoles of different molecules

46
Q

What are London Forces?

A

Weak IMF’s that exist between all molecules

47
Q

How are induced dipole-dipole interactions formed?

A

Moving electrons cause the electron density to fluctuate, which forms temporary dipoles, which cause dipoles to form in neighbouring molecules as they attract one another

48
Q

What is a Van der Waal force?

A

Permanent and induced dipole-dipole interactions

49
Q

What are permanent dipole- dipole forces?

A

Forces that are stronger than London forces between molecules with a polar bond

50
Q

What is a hydrogen bond?

A

Permanent dipole-dipole interaction between a hydrogen atom and the 3 most electronegative atoms

51
Q

What are the properties of a hydrogen bond?

A

-high mp
-results in ice having a lower density than water as they hold molecules in a rigid structure with lots of air gaps

52
Q

What is the solubility of simple molecular structures?

A

-non polar are soluble in non polar
-simple molecular are insoluble in polar
-polar dissolve in polar

Chemistry Topic 2 (5 decks)

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