Properties Of Elemements and trends on the Periodic Table

Question 1

What are the main properties to focus?

Answer 1

Atomic radius -how big the atoms are
Ionisation energy-the amount of energy needed to remove electrons

Electronegativity-how much attraction an atom is an element has for a pair of covalently bonded electrons

Question 2

What is group 7

Answer 2

The halogens

Question 3

Group 0 is…

Answer 3

The noble gases

Question 4

What does the radius of an atom dependent on

Answer 4

The number of protons in the nucleus

The number of shells

Question 5

What is the trend down a group in atomic radius

Answer 5

With each element you have one extra shell o electrons. This means the atoms are getting bigger and bigger with that extra shell, therefore the atomic radius increases down a group

Question 6

Why does the elements across a period increase

Answer 6

The number of protons increase as do the number of electrons but the electrons are filling into the same shell. The increasing number of protons causes an increasing attraction from the nucleus which pulls the shells closer and closer causing the atomic radius to decrease across a period

Question 7

What is the ionisation energy

Answer 7

Refers directly to the energy needed to remove electrons.

For some elements ionisation is quite easy and the would have low ionisation energy.

Others it is easy to remove an electron and hence have the higher ionisation energy

Question 8

Ionisation energy of an element depends on

Answer 8

The atomic radius
The nuclear charge
The number of shells

Question 9

What is the clear trend down a group referring to ionisation energy

Answer 9

When you go down a group both the atomic radius and amount of shells increase meaning the outer shell electrons are feeling less of the attractive force from the nucleus so it can be lost more easily. This results in the ionisation decreasing down a group

Question 10

What is the clear trend across a period referring to ionisation

Answer 10

The nuclear charge is increasing and the atomic radius is getting smaller because the outer shell gets pulled closer to the nucleus. This means the outer electrons are feeling a stronger attraction form the nucleus making it harder for them to be lost. Making the ionisation increase across a period

Question 11

What are the three ways in which the periodic table is arranged

Answer 11

In vertical columns called groups
In horizontal rows called periods
Into 4 blocks

Question 12

What does the nucleus consist of

Answer 12

Positively charged protons,neutrons with no charge negatively charged electrons

Question 13

What is the atom mass and what is the mass number

Answer 13

The larger number is the mass number or atomic and the bottom number is the atomic number

Question 14

How can we just get the mass number

Answer 14

The total amount of protons and neutrons

Question 15

What gives us the atomic number

Answer 15

Number of protons only

Question 16

What is an isotope

Answer 16

Atoms of the same element with a different number of neutrons

Question 17

Give an example of an isotope

Answer 17

The most common had 6 protons 6 elections and 6 neutrons

Question 18

What is isotopic abundance

Answer 18

The relative amount of each isotope found in a sample of a given element

Question 19

What is the relative atomic mass

Answer 19

The mean mass of an atom of an element compared to 1/12th of the mass of the carbon-12 isotope

Question 20

How can we Calculate the relative mass

Answer 20

RAM = sum of (isotopic abundance x mass number )/100

Question 21

What is the most electronegative element on the period table

Answer 21

FLUORINE

Question 22

Why is fluorine the most electronegative element

Answer 22

This means that a fluorine atom in a covenant bond will have the strongest attraction for the electrons in that bond

Question 23

Name some trends and properties in the S-Block

Answer 23

Elements in the s-block are all metals

Ionisation energy decreases down both groups,but group 2 is higher than group of

Atomic radius increases down both groups but group 2 is smaller than group 1

Question 24

Trends and properties in the d-block

Answer 24

D-block elements are all metals as so with the s-block they have the general properties you associate with metals

Question 25

What is the definition of transition metal

Answer 25

An element in the d-block that has at least one ion with an incomplete d-subshell

Question 26

Why are transition metals useful

Answer 26

Because they are good catalyst. They can be used to speed up chemical reactions but don’t get use up in the reaction themselves

Question 27

Trends and properties in group 7

Answer 27

Non-metals but their physical properties change

Reactivity decreases down the group as it gets harder to gain an election

Ionisation energy decreases down the group
Electronegativity decreases down the group
Atomic radius increases down the group

Question 28

Trends and properties in group 0

Answer 28

Boiling point increase down the group

They all have little or no electronegativity and very high ionisation energies

Question 29

What is the Avogadro’s number

Answer 29

6.02x10(23)

602,000,000,000,000,000,000,000

Question 30

What is the formula for concentration when you have a mass

Answer 30

Moles=mass/molar mass

Question 31

What is the formula for moles when a solution is involved

Answer 31

Moles=concentration x volume /1000

Question 32

What is the formula for moles when a gas is involved

Answer 32

Moles=volume/24000

Question 33

Moles formula gas is involved

Answer 33

Moles=(pressure x volume)/(gas constant x temperature)

Question 34

What is molar mass

Answer 34

Molar mass or relative formula mass of a compound is the mass of one mole of that substance. This is easily worked out simple by adding up the relative atomic mass of all the atoms in the molecular formula of the compound.

Question 35

What is the empirical formula

Answer 35

The simplest whole number ratio of atoms in a substance