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Higher chemistry > Structure and bonding (3) > Flashcards

Structure and bonding (3) Flashcards

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1
Q

Ionic bond definition

A

The strong electrostatic force of attraction between the positive ion and the negative ion.

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2
Q

Ionic structure

A

Lattice

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3
Q

What does an ionic formula do

A

It shows the simplest ratio of ions and the charges of the ions

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4
Q

Covalent bond definition

A

The electrostatic force of attraction between the positive nuclei and the shared electrons.

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5
Q

Pure covalent bond definition

A

Where the atoms involved in the covalent bond have the same Electronegativity, or less than 0.5 difference, and therefore share the electrons equally and no dipole is formed.

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6
Q

Polar covalent bond definition

A

Where atoms of a covalent bond have a difference in electro negativity of between 0.5 and 1.6 meaning electrons are shared inequally and this causes a permanent dipole

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7
Q

Dipole definition

A

When atoms share electrons inequally due to the difference in Electronegativity of 0.5 or more, therefore causing the atoms to become oppositely charged.

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8
Q

What is the bonding continuum

A

The order of intramolecular bonds between atoms in order of lowest Electronegativity to highest Electronegativity.

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9
Q

Bonding continuum of pure covalent

A

Both non metals and less than 0.5 difference

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10
Q

Polar covalent continuum

A

0.5 to 1.6 and both non metals

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11
Q

Ionic bond continuum

A

More than 1.6 between a metal and non metal , more than 2.0 between non metals .

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12
Q

Covalent molecule melting and boiling point

A

Low

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13
Q

Ionic bond melting and boiling point

A

High

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14
Q

Electrical conductivity ionic bond

A

Conduct in liquid/solution

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15
Q

Electrical conductor covalent bond

A

No

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16
Q

van der Waals forces

A

Intermolecular forces

17
Q

Intramolecular forces examples

A

Pure covalent bond
Polar covalent bond
Ionic bond

18
Q

Types of van der Waals

A

London dispersion forces
Permanent dipole - permanent dipole
Hydrogen bonding

19
Q

London dispersion forces definition

A

The intermolecular force of attraction between atoms or molecules due to a temporary and induced dipole, caused by the movement of electrons and unequal distribution of electrons.

20
Q

London dispersion forces rules

A

The more electrons the stronger the LDF’s are
The larger the molecule the stronger the LDF’s are

21
Q

What type of molecules and atoms have London dispersion forces

A

All that have electrons

22
Q

Permanent dipole - permanent dipole definition

A

The intermolecular force of attraction between polar molecules oppositely charged dipole. (Not on the same molecule)

23
Q

Polar molecules definition

A

An unsymmetrical molecule containing a dipole.

24
Q

Hydrogen bonding definition

A

The intermolecular force of attraction between the small hydrogen atom and an atom of high Electronegativity such as oxygen nitrogen or fluorine. (Not within the same molecule)

25
Q

Hydrogen bonding atoms

A

Nitrogen, oxygen and fluorine

26
Q

Hydrogen bonding rules

A

The hydrogen must be directly bonded to the other atom
The more examples of hydrogen bonding in the molecule the stronger the hydrogen bonding.

27
Q

van der Waals strength scale

A

Hydrogen bonding
Permanent dipole - permanent dipole
London dispersion forces

28
Q

Why is water denser than ice

A

Because when water freezes the strong hydrogen bonds create a spacious hexagonal structure, whereas in water the molecules are pulled very closer together.

29
Q

What do polar substances dissolve in

A

Polar solvents

30
Q

What do non polar substances dissolve in

A

Non polar solvents

31
Q

What do ionic substances dissolve in

A

Polar solvents

32
Q

What do hydrogen bonded substances dissolve in

A

Hydrogen bonded solvents

33
Q

How do ionic substances dissolve

A

The polar solvents will break apart the lattice and surround their oppositely charged ion.

34
Q

Viscosity rule

A

The stronger the intermolecular forces, the stronger the viscosity

35
Q

Polar experiments

A

Put the solvent next to a charged rod and see if it bends

36
Q

Viscosity experiments

A

See how long an air bubble travels to the bottom of the tube with the liquid in.

37
Q

Unique feature of water

A

Surface tension
(Hydrogen bonding)

Higher chemistry (10 decks)

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