The Particulate Nature of Matter

Question 1

does gas and liquid have a fixed shape?

Answer 1

no, only solid have fixed shapes

Question 2

describe the movement of particles in liquids?

Answer 2

particles slide past each other

Question 3

describe the movement of particles in gases?

Answer 3

particles move rapidly and randomly

Question 4

what are the states of matter?

Answer 4

solid, liquid and gas

Question 5

describe the movement of particles in a solid?

Answer 5

particles vibrate about a fixed position

Question 6

describe the arrangement of particles in a liquid?

Answer 6

• closely packed
• disorderly manner

https://tse4.mm.bing.net/th?id=OIP.AxYNKAX_FJcxiDYXxZk31QHaD2&pid=Api&P=0&h=180

Question 7

describe the arrangement of particles in a solid

Answer 7

• very closely packed
• orderly manner

https://tse4.mm.bing.net/th?id=OIP.AxYNKAX_FJcxiDYXxZk31QHaD2&pid=Api&P=0&h=180

Question 8

describe the arrangement of particles in a gas?

Answer 8

• disorderly
• very far apart

Question 9

attractive forces between particles of a solid?

Answer 9

very strong

Question 10

attractive forces between particles of a liquid

Answer 10

strong

Question 11

attractive forces between particles in a gas

Answer 11

very weak

Question 12

Guidelines to draw particles

Answer 12

• At least 75% of space should be covered
• At least 9 particles drawn (for solid & liquid states)
• Minimum 3 for gaseous state
• All particles are to be of the same size
• Space between any 2 particles should be smaller than the size of 1 particle

Question 13

What is the relative charge and mass of a proton?

Answer 13

relative charge: +1
relative mass: 1

Question 14

What is the relative charge and mass of a Neutron?

Answer 14

relative charge: 0
relative mass: 1

Question 15

What is the relative charge and mass of a Electron?

Answer 15

relative charge: -1
relative mass: 1/1840

Question 16

What is sublimation?

Answer 16

We can define sublimation as the transition of a substance from the solid phase to the gaseous phase without changing into the liquid phase.

Question 17

define proton (atomic) number

Answer 17

The number of protons in the atom

Question 18

Define mass number/Nucleon Number

Answer 18

The total number of protons and neutrons in the atom.

Question 19

What do you notice about the number of protons and electrons

Answer 19

The number of protons is equal to the number of electrons

Question 20

What are the electrons in the outermost shell called?

Answer 20

Valance electrons

Question 21

define the term isotopes

Answer 21

Atoms of the same element with the same number of protons and electrons but different number of neutrons.

Question 22

Describe how a magnesium
atom forms a magnesium ion.

Hint: how to make to stable electronic configuration?

Answer 22

Electronic structure of magnesium is 2.8.2.
It will lose 2 electrons Ion to form Mg2+ ion and obtain stable electronic configuration
Ionic Equation Mg  Mg2+ + 2e-

Question 23

What are noble gases?

Answer 23

Noble gas: group 0 ,
monoatomic gas ,
stable electronic configuration

Question 24

Do metals gain or lose electrons?

hint: picture the periodic table in ur head, how to make metals stable?

Answer 24

metals lose electrons

Question 25

Do non-metals gain or lose electrons? | hint: picture the periodic table in ur head, how to make metals stable?

Answer 25

gain electrons

Question 26

What is an ionic bond?

Answer 26

It is formed by transfer of electrons from metal to non metal

Question 27

What is covalent bond?

Answer 27

Sharing of electrons between non metals

Question 28

How is the bond in sodium chloride formed? (use this structure to do other similar qns)

Answer 28

Electronic configuration > Electronic configuration of sodium is 2.8.1 and chlorine is 2.8.7. Process > Sodium atom will transfer 1 valence electron and the Chlorine atom will gain 1 electron Ion > Sodium will form +1 charge and chloride ion -1 charge Reason> To obtain stable electronic configuration

Question 29

MUST KNOW covalent structures!

Answer 29

- water - Ammonia - Carbon Dioxide - Methane note to self: add in picture from pg 5 chapter 10 bonding

Question 30

When to draw ionic compound?

Answer 30

When metal and non-metal transfer electrons

Question 31

when to draw covalent compound?

Answer 31

when non-metal and non-metal shares electrons

Question 32

What are the physical properties of ionic compound?

Answer 32

- Ionic bonds are formed by transfer of electrons from metals to non metal - Metal atoms tend to lose electrons to form positive ions. (cations) - Non-metal atoms tend to gain electrons to form negative ions. (anions)

Question 33

properties of Ionic compounds

Answer 33

- High melting and boiling point Structure > Giant lattice structure Attraction > Strong electrostatic forces of attraction between Particles >Opposite charged ions Energy > More energy needed to break these forces

Question 34

Properties of Covalent compound

Answer 34

- Low melting and boiling point Structure >Simple molecular structure Attraction >Weak intermolecular forces of attraction between Particles> molecules Energy>Less energy needed to break these forces

Question 35

State of ionic compound at room temp.

Answer 35

Solids at room temp.

Question 36

State of covalent compound at room temp.

Answer 36

usually exist as gases or liquids at room temperature

Question 37

Solubility of Ionic compounds

Answer 37

- soluble in water - insoluble in organic solvent eg. Oil, alcohol

Question 38

Solubility of Covalent compounds

Answer 38

- soluble in organic solvent - insoluble in water

Question 39

Electrical Conductivity of ionic compounds

Answer 39

In molten and aqueous states Reason: Mobile ions are present as able to move and carry electric current

Question 40

Electrical Conductivity of covalent compounds

Answer 40

Does not conduct electricity in any state Reason: No mobile ions to carry electric current

Question 41

Why are ionic compounds unable to conduct electricity in a solid state?

Answer 41

Ions are held in fixed positions in a giant ionic lattice structure and unable to move

Question 42

Covalent compounds cannot conduct electricity in any state, but there are Exceptions

Answer 42

Hydrogen chloride gas dissolves in water to form hydrochloric acid. In aqueous state, ions are able to move & carry electric current Equation: HCl (aq) >H+(aq) + Cl- (aq)

Question 43

Using structure and bonding, explain why the melting point of sodium chloride (ionic compound) is higher than chlorine gas (covalent compound)? | hint: use SAPE to answer the qn

Answer 43

Sodium chloride has giant lattice structure (S) with strong electrostatic forces of attraction between (A) opposite charged ions (P) More energy needed to break these forces (E). Chlorine has has simple molecular structure (S) weak intermolecular forces of attraction between(A) molecules (P). Less energy needed to break these forces.(E)