Section A
Atomic Structure
Atoms are the building blocks of all matter. They are made of protons (+ charge, in nucleus), neutrons (no charge, in nucleus), and electrons (- charge, orbiting nucleus). Atomic number = number of protons. Mass number = protons + neutrons.
Click to explore atom structure
Hydrogen: 1 proton, 0 neutrons, 1 electron
Q1
What is the atomic number of an atom?
1 mark
Q2
What is the mass number of an atom?
1 mark
Q3
A carbon atom has 6 protons, 6 neutrons, and 6 electrons. What is its mass number?
1 mark
Q4
An atom has atomic number 17 and mass number 35. How many neutrons does it have?
2 marks
Q5
Which subatomic particle has a negative charge?
1 mark
Q17
In the notation 2311Na for a sodium atom, what do the numbers 23 and 11 represent, in order?
1 mark
ATOMIC STRUCTURE — SECTION SCORE
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Section B
Electronic Structure
Electron shells: Electrons orbit the nucleus in shells, also called energy levels. The first shell holds up to 2 electrons, the second up to 8, the third up to 8 (for elements 1-20). Electronic structure shows how electrons are arranged, e.g., Carbon (6 electrons) = 2,4.
A bit of history: in 1913, Danish scientist Niels Bohr built on Ernest Rutherford's model of the atom, showing that electrons move in different energy levels around the nucleus rather than anywhere at random. Bohr was awarded the Nobel Prize for this work, and it's still the model we use today.
Q6
What is the electronic structure of a sodium atom (atomic number 11)?
2 marks
Q7
A chlorine atom has atomic number 17. What is its electronic structure?
2 marks
Q8
How many electrons are in the outer shell of a fluorine atom (atomic number 9)?
1 mark
Q16
How is Bohr's model of the atom different from Rutherford's model?
1 mark
Q18
Electron shells fill from the shell closest to the nucleus outwards. What is the maximum number of electrons that can occupy the first three shells, in order?
1 mark
ELECTRONIC STRUCTURE — SECTION SCORE
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Section C
The Periodic Table
The Periodic Table organizes all known elements by atomic number. Groups are vertical columns (elements with similar properties). Periods are horizontal rows (elements with the same number of electron shells). Metals are on the left and centre, non-metals on the right.
Click on any element to select it
123456789101112131415161718
H
1
He
2
Li
3
Be
4
B
5
C
6
N
7
O
8
F
9
Ne
10
Na
11
Mg
12
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Q9
In the periodic table, elements in the same group have what in common?
1 mark
Q10
In the periodic table, elements in the same period have what in common?
1 mark
Q11
Which group contains the noble gases?
1 mark
PERIODIC TABLE — SECTION SCORE
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Section D
Properties & Trends
Metals (left of the zig-zag line) are shiny, malleable, ductile, conduct heat/electricity, and have high melting points. Non-metals (right of the zig-zag line) are dull, brittle, poor conductors, and have lower melting points. Going down a group, atomic size increases and reactivity increases for metals, decreases for non-metals.
Q12
Which of these is a metal?
1 mark
Q13
Which of these is a non-metal?
1 mark
Q14
What happens to atomic size as you go down a group in the periodic table?
1 mark
Q15
Which element in Group 1 is the most reactive?
2 marks
PROPERTIES & TRENDS — SECTION SCORE
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