Atomic structure and the periodic table T1

Question 1

What are the 3 subatomic particles?

Answer 1

Protons, neutrons and electrons

Question 2

What are protons?

Answer 2

They are heavy and positively charged

Question 3

What are neutrons?

Answer 3

Neutrons are neutral and heavy

Question 4

What are electrons?

Answer 4

Electrons have hardly any mass and are negatively charged

Question 5

What is an atom?

Answer 5

Atoms are neutrally charged which means that they have the same amount of protons as electrons

Question 6

What are isotopes?

Answer 6

Isotopes are different forms of the same element, which have the same number of protons but a different number of neutrons

Question 7

What is the relative atomic mass?

Answer 7

The relative atomic mass of an element is the average mass of one atom of the element, compared to 1/12 of the mass of one atom of carbon-12

Question 8

What are isotopic abundances?

Answer 8

Different isotopes of an element which occur in different quantities

Question 9

How do you work out relative atomic mass using isotopic abundances?

Answer 9

Multiply each relative isotopic madd by its isotopic abundance, and add up the results. Divide that by the sum of the abundances ( if the abundances are given as percentages, this will be 100)

Question 10

In what year did Dmitri Mendeleev create the table of elements?

Answer 10

1869

Question 11

How did Mendeleev order his table?

Answer 11

In order of atomic mass, he then discovered a pattern where her could put elements with similar chemical properties in columns

Question 12

What is the difference between the table of elements and the periodic table?

Answer 12

The rows are now periods which show how many shells an element has

Question 13

How do you work out electronic configuration of an element from its period and group?

Answer 13

The number of shells which contain electrons is the same as the period of the element and the group number tells you how many electrons occupy the outer shell of an element