Atomic Structure

Question 1

What is the relative mass for proton, neutron and electron?

Answer 1

In proton, 1
In neutron, 1
In electron, 0

Question 2

What is the relative charge for proton, neutron and electron?

Answer 2

In proton, +1
In neutron, 0
In electron, -1

Question 3

What is orbital?

What is the 4 types?

Answer 3

is a subshell which have different energy state

s,d,pf

Question 4

Aufbau principle?

Answer 4

its state that the electrons fill the orbitals wth lowest available energy state before filling orbitals with highest available energy state

Question 5

Bohr Model?

Answer 5

Describe the shape in space where electrons can be found in atoms

Question 6

What is electronic configuration?

Answer 6

Is the distribution of an electrons in an atom

Question 7

Electronic configuration: 1s, 2s…….

each letter contains how many
S- P- D-

Answer 7

2p, 3s, 3p, 4s, 3d, 4p, 4d

2 6 10

Question 8

Type of element in each group?

Answer 8

Group 1- Alkali metals
2- Alkali earth metals
3-11- transition metals
17- Halogens
18- Noble gases

Question 9

Ionic Bonding?

Answer 9

is an electrostatic attraction betweem 2 oppositely charged ions

Question 10

What type of bonding this is?

Answer 10

Ionic bonding

Question 11

What is an electrostatic attraction?

Answer 11

Is the force experience by oppositely charged particles

Question 12

What happen to electrostatic force when the ionic increases

Then what happen when ionic radius increases

Answer 12

It gets stronger

It gets weaker

Question 13

What is covalent bonding?

Answer 13

Is an electrostatic attraction between shared pair of electrons and nuclei bonded atom

Question 14

What is dative covalent bond

Answer 14

Also known as multiple bonds

Occurs when both sharing electrons come from 1 atom

Question 15

What is a lone pair? How it can be created?

Answer 15

A pair of non-bonded atom

It can be created when an lobe pair bind to other ions

Question 16

What type of bonding this is

Answer 16

Covalent bonding

Question 17

What is an organic compound?

Answer 17

Is a compound contain one ormore carbon in an carbon chain

Question 18

Atoms that’s bonded covalently has?

Answer 18

great lattice structure and high melting point

Question 19

What is metallic bonding?

Answer 19

Is a bond between metals only

Question 20

Metallic bonding has?

Answer 20

Delocalised electrons amd are free to move

Question 21

Metals properties? Why?

Answer 21

Good conductor- cuz of delocalised electrons moving freely

High melting and boiling point- cuz of strong electrostatic attraction

Malleable- a layer of positive ion slide on each other and delocalised electrons move with layer

Ductile- a postive ion roll over each other and delocalised electron move with positive ion

Question 22

Why melting point in group 1 decreases

Answer 22

as the atoms get larger the more electron it’ll be thereby more shell this means that there’s more shielding between nucleus and delocalised electrons, so the electrostatic attraction gets weaker producing weak metallic bond

Question 23

Why melting point group 2 is higher than group 1

Answer 23

Because group 2 contains 2 delocalised electrons which gives greater electric density. The +2 charge produces stroger electrostatic attraction between nucleus and delocalised electrons producing stronger metallic bonding

Question 24

What is an intermolecular force?

All intermolecular forcr are what?

Answer 24

Is an attraction between molecules caused by either permanent or temporary induce dipole

Vaderwaals forces

Question 25

What is london forces?

Answer 25

A force that only exist between noble gases and non-polar molecules Electrons move randomly in a shell of a molecule causing even distribution, causing temporary dipole which can induce a temporary dipole in another molecule

Question 26

What forces is this?

Answer 26

London forces

Question 27

What is dipole-dipole forces? What is polar molecules

Answer 27

Is an forces between polar molecules Polar molar has permanent positive and negative end, which attracted at each other

Question 28

What force is this

Answer 28

Dipole-Dipole forces

Question 29

What is the strongest form of intermolecular forces

Answer 29

Hydrogen bond

Question 30

How hydrogen bond is form

Answer 30

Hydrogen bond form when compound have hydrogen bounded with flourine, oxygen and nitrogen

Question 31

How to get Mass (g)

Answer 31

Mass= molar mass (g mol-1) x no. of moles (mol)

Question 32

How to get emperical formula?

Answer 32

1. Mass/grams is given 2. Find the molecular mass of the elements 3. Divide the mass to the molecular mass 4. Whatever the lowest will be divided to the answer 5. Then put the number you get to the symbols

Question 33

How to get relative atomic mass?

Answer 33

Find the atomic mass and add it altogether

Question 34

How to get expected mass?

Answer 34

Calculate the RAM for everything Then, divide the RAM of the question to the RAM given Next is multiply it to the mass given

Question 35

How to get molar concentration (mol dm-3) ?

Answer 35

Amount, N (mol) ÷ Volume (dm-3) DON'T FORGET CONVERSION OF CM^3 TO DM^3 (÷1000)

Question 36

How to calculate percentage yield?

Answer 36

%= actual amount (mol) of product ÷ theorethical amount (mol) of product Calculate molar mass first Calculate no. of moles of given by mass÷molar mass Theoretical number of moles of queastion by ration like (1:1 or 1:2) Calculate the actual no. of moles of queastion by mass÷molar mass Divide the actual no. of moles to theoretical one then multiply by 100

Question 37

How to get theoretical yield

Answer 37

Molar mass of element they're asking No. of moles of the given element by mass (g) ÷ molar mass (g mol-1) No. of moles multiply to molar mass of the question they're asking

Question 38

Trends in periodic table:

Answer 38

Group 1-0 indicates the no. of electron in their shell for each element in the group Period 1-7 indicates the main level energy of each element in the period s,p,d block indicates sub shells being filled with electrons

Question 39

What is first ionsation energy? As you go down the group what happen to ionisation energy

Answer 39

Is the minimun energy needed for 1 mole of electrons should/to be removed from 1 gaseos atom The ionisatiom energy decreases ad the outer electron being removes is further from the nucleus and no more inmer shell to shield the outer electrons

Question 40

What is electron affinity?

Answer 40

An atom ability to gain an electron and become NEGATIVE ion Example; O (g) + e- --------> O- (g)

Question 41

What is electronegativity? What is the most electronegative element?

Answer 41

Is a measure of tendency of an atom to attract a bonded pair of electrons Fluorine Increases as you go across the group Decreases as you go down the group

Question 42

Structure, Forces and Bonding of period 2 and 3

Answer 42

Li, Be, B, Na, Mg, Al are giant metallic structure, Strong forces between positive ions and delocalised electrons and Metallic Bonding C, Si is a Giant covalent structure, Strong forces between atoms and Covalent bonding

Question 43

Melting and Boiling point Trends:

Answer 43

Going down group 1 the m. and b. point decreases which means that the forces of attraction gets weak Down group 7 the m. and b. point increases which means that the forces of attraction gets stronger Non-metals in group 3-7 have low melting point

Question 44

Products and reactivity of with oxygen

Answer 44

Group 1 metal reacts rapidly with oxygen Group 2-4 metals burn in oxygen forming metal oxide

Question 45

Products and reactivity of metals with water

Answer 45

Group 1 react with water producing basic alkaline solution Group 2 reacts with water produce hydroxide Group 3 is very reactive is very water Group 4-6 does not react with water

Question 46

Products and reactivity of metals with dilute HCL and diluye sulfuric acid

Answer 46

Metals react with dilute acid forming metal salts and hydrogen As you go down the group the metals will become more reactive As you go across the period the metals become less reactive

Question 47

Reactivity of the position of metals

Answer 47

Most reactive in group 1 Then group 2, 3, 4 then....... More reactive can easily attract electrons as there's less shield to the nucleus, increasing the force of attraction

Question 48

What is oxidation and reduction

Answer 48

Oxidation- loss of electron. Increase of oxidation number Reduction-gain of electrons. Decrease of oxidation number

Question 49

How atom becomes an ion?

Answer 49

When atom loses or gain electron

Question 50

Oxidation rules!!!!

Answer 50

``` Element- 0 Fluorine in a compound- (-1) Oxygen- (-2) Hydrogen - (+1) unless bonden with metals (-1) Chlorine, bromine and iodine- (-1) except bonded with oxygen Group 1 metals- +1 Group 2 metals- +2 Aluminium - +3 ```

Question 51

What is transition metals?

Answer 51

A d-block element which forms at least one stable ion with incomplete d-subshell

Question 52

Displacement of metals and halogens

Answer 52

A metal will displace less reactive metal Form ion metal- metal atom lose electron and so are oxidised Form atom- metal ion gain electron so are reduced

Question 53

Uses and application of substances

Answer 53

Metal oxide- used as a starter material for industrial processes such as fibre glass Metal salt- used to make colours in fireworks Sodium chloride- used in manifacturing processes such as making paper or glass Sulphate- used in detergents Copper sulphate- used in water treatment to kill algae