Ni

Question 1

3 states of matter

Answer 1

Solids liquids gases

Question 2

Gases have no what (2)

Answer 2

Fixed volume or shape and move around freely

Question 3

Solids and liquids particles are

Answer 3

Tightly packed together

Question 4

What condense and freeze at sufficiently low temperatures

Answer 4

Molecular element

Compounds

Monatomic elements

Question 5

For freeze and condense what must occur

Answer 5

Forces of attraction between discrete atoms or molecules

=VDWF

Question 6

What are LDF

Answer 6

Forces of attraction that can operate between all atoms & molecules

Question 7

Are they weak or strong LDF

Answer 7

Much weaker than all other types of bonding

Question 8

Strength of LDF depends upon what

Answer 8

•No of e
More e the stronger intermolecular forces

Question 9

Why are LDF formed?

Answer 9

As a results of electrostatic attraction between TD and induced dipoles & induced dipoles causes by movement of E in atoms or molecules

Question 10

Dipoles occur when

Answer 10

A dipole in a molecule occurs when opposite ends of atoms, molecules or compounds have different e charged

Question 11

What affect can dipoles have on their neighbouring atoms

Answer 11

Attract atoms e to other end so another dipole is made

Question 12

The uneven distribution of electrons are only

Answer 12

Temporary

Temporary due to small and temporary they are very weak

Question 13

The negative end of an atom will what (dipole)

Answer 13

The repel -E on adjacent atoms causing T.D called induced dipoles

Question 14

So what’s the positive end like of a dipole

Answer 14

It’s attracted to the - end of the dipole on a nearby atom

Question 15

Non polar covalent bonds

Answer 15

•occur between non metals with same E.N
•The more e, the stronger LDF, the more energy to break
•LDF are their intermolecular forces

Question 16

Covalent bond occurs

Answer 16

Between non metal atoms with slightly different electronegative values

Question 17

In a polar covalent bond what isn’t shared equally

Answer 17

•Electrons aren’t shared equally due to EN values

Question 18

Where do the electrons sit closer to

Answer 18

The atom with the higher electronegative values as it has a stronger attraction for shairrd pair of e

Question 19

What does difference in electronegative values cause

Answer 19

Atoms to be slightly charged

Question 20

The - dipole in molecules is electrostaticlly

Answer 20

Attracted to the + Dipole

Question 21

Covalent bond definition

Answer 21

Electrostatic force of attraction of positively charged non-metal nuclei for a shaired pair of electrons

Question 22

In polar dipoles what are present (bonding)

Answer 22

PD

Question 23

What is a permanent dipole?

Answer 23

A PD is a Permanent persistent uneven distribution of electrons due to their diffuclut in e.n between atoms in a molecule, resulting in asymmetrical charged dipoles

Question 24

1 atom attracts what in a PD

Answer 24

Attracts e more than the other becoming more -

Question 25

The more E.N the more?

Answer 25

More polar

Question 26

Types of VDWF

Answer 26

HB PDPDI LDF

Question 27

Hydrogen bond is a form of what

Answer 27

PDPDI

Question 28

What are hydrogen bonds

Answer 28

Electrostatic forces of attraction between molecules that contain these highly polar bonds

Question 29

Hydrogen bonds are when we see

Answer 29

O-H N-H F-H

Question 30

Bonds consisting of hydrogen atom bonded to an atom of

Answer 30

Strongly electro negative elements As mentioned n,O,F

Question 31

A hydrogen bond is the strongest buy weaker compared to an

Answer 31

Covalent bond

Question 32

Anomalous boiling points of ammonia eg water and fluoride are a result of

Answer 32

HB

Question 33

Metallic bonding contains what’s

Answer 33

Metals

Question 34

Is metal bonding strong or weak

Answer 34

Strong

Question 35

Structure of metallic binding

Answer 35

Electrostatic attraction between the positive ions & the sea of delocalised electrons

Question 36

Why are metallic boiling points high

Answer 36

Due to large amount of energy needed to break the string metallic bonds Except mercury

Question 37

Across a period metallic bonding

Answer 37

The nuclear charge increases causing the electrons become strongly attracted to the nucleus. This means more energy is required to break the attractions hence the higher melting and boiling points.

Question 38

Metallic Bonding down period

Answer 38

Down a group the number of electron shells increases meaning the outer electrons are further away from the nucleus therefore less strongly attracted This week attractions require less energy to be broken, hence the decrease in melting and boiling points

Question 39

Why are monotonic single atoms?

Answer 39

Due to them having full outer electron shells making them stable

Question 40

What is a covalent networks structure

Answer 40

A covalent network structure contains a giant lattice of non-metals atoms bonded by strong covalent bonds

Question 41

3 elemental covalent structuresb

Answer 41

Silicon = 4 atoms = spider Boron = 3 atoms = hexagon Carbon= Diamond & graphite

Question 42

Why do elements covalent bonds have a very high melting and boiling point

Answer 42

Due to large need to break strong covalent bonds that require large amounts of energy to breaks

Question 43

Why is graphite different in structure

Answer 43

Because: •carbon atoms form layers of hexagonal rings • these rings are held together by LDF, as the forces between them are weaker then covalent bonds it allows layers to slide across each other.

Question 44

What are molecules And what are covalent molecular substances made out of

Answer 44

•Group of atoms helps together by covalent bonds Covalent molecular substances are made up of LDF between molecules that are weak •

Question 45

Ionic bond structure

Answer 45

•formed between at least 1 metal and non metal ion

Question 46

What is ionic bonding

Answer 46

It’s the e.s attraction between a positively charged metal ion and a negatively charged non metal ion

Question 47

Difference in electronegativity ruling for polar

Answer 47

Polar bond formed if difference in e.n is between 0.1-0.8

Question 48

Ionic bonding fomed when EN

Answer 48

Difference greater then 1.8 These are ballpark figutes

Question 49

Viscosity

Answer 49

Measure of how thick a liquid is or how slow it moves

Question 50

Slower IMF viscosity results in

Answer 50

Slows liquid, greater viscosity This mean substances with HB will be most viscous LDF= less viscosity V= no of e depending

Question 51

Solubility meaning

Answer 51

Ability of a substance to dissolve in a substance

Question 52

Aquesos and non aquesos is what

Answer 52

Polar Non-polar

Question 53

“Like to dissolve like”

Answer 53

Polar substances dissolve in polar solvents

Question 54

What are polar compounds attracted to each other

Answer 54

Due to PD.