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Flashcards in Bonding Deck (23)
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1

What is ionic bonding

Strong electrostatic forces of attraction between oppositely charged ions held in a lattice

2

Ionic bp

High because takes a lot of energy to break strong electrostatic forces of attraction between oppositely charged ions

3

Do ionic compounds conduct electricity

Yes when molten as ions are free to move

4

What is simple molecular covalent bonding

Strong covalent bonds between atoms, weak van der waals forces of attraction between molecules

5

Can simple molecular covalent molecules conduct electricity

No, no electrons free

6

So simple molecular substances have a high or low bp

Low
Weak van der waals forces of attraction between molecules that don’t take much energy to overcome

7

Describe macromolecular covalent bonding

Lattice of many atoms held together by strong covalent bonds

8

So macromolecular covalent bonds have high or low bp

High
As it takes a lot of energy to overcome strong covalent bonds

9

Metallic bonding

Lattice is positive metal ions strongly attracted to a sea of delocalised electrons

10

Do metallic compounds have a high or low bp

High
Strong forces of attraction between positive ions and negative electrons

11

Do metallic compounds conduct electricity

Yes as delocalised sea is electrons

12

Define electronegativity

The ability of an atom to attract the pair of electrons in a covalent bond

13

What affects electronegativity

Nuclear charge
Atomic radius
Electron shielding

14

What is the most electronegative element

F

15

How do you get a non polar bond

Both bonding elements have the same electronegativities

16

What is the strongest intermolecular force

Hydrogen bonding

17

What is the weakest intermolecular force

Van der waals

18

Describe van der waals

Temporary dipoles are created by the random movement of electrons
Induces dipole in neighbouring molecule
Temporary induced dipole dipole

19

Describe permanent dipole dipole

Some molecules with polar bonds have permanent dipoles
Forces of attraction between those dipoles and those of neighbouring molecules

20

What conditions are needed for hydrogen bonding

O N F are highly electronegative
Strong attraction between H nucleus and lone pair of electrons on O N F

21

Why is ice less dense than liquid water

In liquid hydrogen constantly break and reform
In ice the hydrogen bonds hold the molecules in fixed positions this makes them slightly further apart than in liquid

22

What is co ordinate bonding

Formed when an electron deficient atom accepts a lone pair of electrons from an atom with a lone pair of electrons

23

What does the shape of molecules depend on

Number of electrons on the valence shell
Number of these electrons which are in bonded or lone pairs