A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes

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Question 31

Medium

Complete the sentences. Choose answers from the box. Each word may be used once, more than once, or not at all.

electron
ion
neutron
nucleus
proton

J.J. Thomson's plum pudding model was disproved when alpha particles were deflected by a dense, central ____________________.
James Chadwick discovered this uncharged subatomic particle in the nucleus: the ____________________.
Niels Bohr suggested that these negative particles orbit the nucleus at specific distances (energy levels): the ____________________.
The atomic number, which defines each distinct element, represents the number of this positive particle: the ____________________.
When a neutral atom gains or loses electrons, it becomes a charged species known as an ____________________.

[5]

Table 1 shows information about two isotopes of element $Z\text{Z}$ .

	Mass number	Percentage (%) abundance
Isotope 1	20	90
Isotope 2	22	10

Calculate the relative atomic mass ( $A_r$ ) of element $Z\text{Z}$ using the equation:

$2100A_r = \frac{(\text{mass number} \times \text{percentage}) \text{ of isotope 1} + (\text{mass number} \times \text{percentage}) \text{ of isotope 2}}{100}$

Give your answer to 1 decimal place.

[2]

Suggest the identity of element $Z\text{Z}$ . Use the periodic table.

[1]

The radius of an atom of element $Z\text{Z}$ is $1.6 \times 10^{-10}\text{ m}$ .

The radius of the nucleus of the atom is $000\frac{1}{100\,000}$ of the radius of the atom.

Calculate the radius of the nucleus of an atom of element $Z\text{Z}$ . Give your answer in standard form.

[2]

A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46

Question 31

Medium

Complete the sentences. Choose answers from the box. Each word may be used once, more than once, or not at all.

electron
ion
neutron
nucleus
proton

J.J. Thomson's plum pudding model was disproved when alpha particles were deflected by a dense, central ____________________.
James Chadwick discovered this uncharged subatomic particle in the nucleus: the ____________________.
Niels Bohr suggested that these negative particles orbit the nucleus at specific distances (energy levels): the ____________________.
The atomic number, which defines each distinct element, represents the number of this positive particle: the ____________________.
When a neutral atom gains or loses electrons, it becomes a charged species known as an ____________________.

[5]

Table 1 shows information about two isotopes of element $Z\text{Z}$ .

	Mass number	Percentage (%) abundance
Isotope 1	20	90
Isotope 2	22	10

Calculate the relative atomic mass ( $A_r$ ) of element $Z\text{Z}$ using the equation:

$2100A_r = \frac{(\text{mass number} \times \text{percentage}) \text{ of isotope 1} + (\text{mass number} \times \text{percentage}) \text{ of isotope 2}}{100}$

Give your answer to 1 decimal place.

[2]

Suggest the identity of element $Z\text{Z}$ . Use the periodic table.

[1]

The radius of an atom of element $Z\text{Z}$ is $1.6 \times 10^{-10}\text{ m}$ .

The radius of the nucleus of the atom is $000\frac{1}{100\,000}$ of the radius of the atom.

Calculate the radius of the nucleus of an atom of element $Z\text{Z}$ . Give your answer in standard form.

[2]

A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes

Question 31

A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Questions

A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes

Question 31

A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Questions