C3.1

Question 1

Where has the modern periodic table been developed from

Answer 1

Work begun by Newlands and mendeleev

Question 2

What are the trends in chemical properties within the periodic table linked to

Answer 2

How easily the element gains or loses electrons

Question 3

What did newlands and then mendeleev attempted to do

Answer 3

Classify the elements by arranging them in order of their atomic weights

Question 4

How can the periodic table list be arranged

Answer 4

In a table so that elements with similar properties are in columns, known as groups

Question 5

Why is the periodic table called the periodic table

Answer 5

Because similar properties occur at regular intervals

Question 6

What was wrong with the early periodic table

Answer 6

It was incomplete and some elements were places in inappropriate groups if the strict order of atomic weights was followed

Question 7

What did Mendeleev overcome

Answer 7

Some of the the problems by leaving gaps for elements that he thought had not been discovered

Question 8

When electrons, protons and neutrons discovered

Answer 8

20th century

Question 9

In the 20th century how was the periodic table arranged

Answer 9

In order of atomic numbers and all the elements were placed in appropriate groups

Question 10

What can the modern periodic table be seen as

Answer 10

An arrangement of the elements in terms of their electronic structures

Question 11

What do elements in the same group have

Answer 11

The same number of the electrons in their highest occupied energy level

Question 12

6 Properties of alkali metals ( group 1)

Answer 12

Low density

First three elements are less dense than water

React with non metals to form ionic compounds with the metal ion has a charge of +1

Compounds are white solids that dissolve in water to form colourless solutions

React with water , releasing hydrogen

Form hydroxides that dissolve in water to give alkaline solutions

Question 13

In group one the further down the group an element is

Answer 13

The more reactive

The lower is melting and boiling points

Question 14

Compared with group 1 elements, transition elements….

Answer 14

Have higher melting points and densities ( except mercury)

Stronger
harder
Less reactive
Do not react as vigorously with water or oxygen

Question 15

What are 3 properties of transition metals

Answer 15

Can be used as catalysts
Have ions with different charges
Form coloured compounds

Question 16

What do halogens react with

Answer 16

Metals to form ionic compounds where the halide ion carries a charge of -1

Question 17

In group 7 the further down the group the element is

Answer 17

The less reactive the element

The higher its melting point and boiling point

Question 18

What can a more reactive halogen do

Answer 18

Displace a less reactive halogen from an aqueous solution of its salt

Question 19

Why can the trends in reactivity within groups in the periodic table be explained

Answer 19

Because the higher the energy level of the outer electrons:
The more easily electrons are lost
The less easily electrons are gained