1.3 Bonding Flashcards Preview

Chemistry AS 2015-16 > 1.3 Bonding > Flashcards

Flashcards in 1.3 Bonding Deck (22)
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1

Which element is most electro positive and why?

Caesium.
Has a large atomic radius with comparatively low nuclear charge.

2

How does electronegativity change across a period and why?

Electronegativity increases.
Because...
Nuclear charge increases
The number of energy levels remains the same
Atoms contract so get smaller

3

Name the three main types of intermolecular force from weakest to strongest.

Van der Waals
Dipole-dipole
Hydrogen bonding

4

What is the shape and bond angle for a molecule with:
3 bonding pairs
1 lone pair

Pyramidal
107 degrees

5

What is the shape and bond angle for a molecule with:
3 bonding pairs
No lone pairs

Trigonal planar
120 degrees

6

What is the shape and lone pair for a molecule with:
4 bonding pairs
2 lone pairs

Square planar
90 degrees

7

What is the shape and bond angle for a molecule with:
4 bonding pairs
No lone pairs

Tetrahedral
109.5 degrees

8

What is the shape and bond angle for a molecule with:
6 bonding pairs
No lone pairs

Octahedral
90 degrees

9

What is the shape and bod angle for a molecule with:
2 bonding pairs
2 lone pairs

Bent
104.5 degrees

10

What is the shape and bond angle for a molecule with:
2 bonding pairs
No lone pairs

Linear
180 degrees

11

What is the shape and bond angle for a molecule with:
5 bonding pairs
No lone pairs

Trigonal bipyramid
120 degrees

12

Which element is most electronegative and why?

Fluorine.
Has a small atomic radius with a comparatively large nuclear charge.

13

What is Electronegativity?

Electronegativity is the relative ability of an atom to attract electrons in a covalent bond.

14

What is Dative bonding?

A Dative covalent bond is a pair of electrons shared between two atoms, one of which provides both electrons to the bond.

15

What is Polar bonding?

A Polar covalent bond is a pair of electrons that are shared unequally between two atoms.

16

Name 4 types of crystal structure

- Ionic
-Metallic
-Macromolecular (giant covalent)
-Molecular

17

What's the structure, type of bonding and properties of DIAMOND.

Giant Molecular
Covalent
Shiny and hard
High melting point
High boiling point

18

What's unusual about graphite?

It conducts electricity due to having delocalised electrons

19

What happens to iodine when heated and why?

It sublimes(goes from solid to gaseous)
Due to the fact only VdW forces are holding iodine atoms together so it's very easy to overcome these forces resulting in a low boiling point.

20

Explain why does ice float?

Water molecules are held together by weak hydrogen bonds.
These hydrogen bonding forces a rather open structure on the ice leaving gaps in the structure. This means that when water freezes it expands which occupies more space becoming less dense that water.

21

Define metallic bonding

Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice.

22

Define ionic bonding

Ionic bonding involves electrostatic attraction between oppositely charged ions in a lattice