Chemistry C1 1.3 The arrangement of elections in atoms.

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What atoms have very stable arrangements of electrons?
All the atoms of the un-reactive noble gases (in Group 0).
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Where are electrons in atoms?
In energy level that can be represented by shells.
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Where are electrons in the lowest energy levels located?
In the shell closest to the nucleus.
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In which order do electrons occupy energy levels?
Electrons occupy the lowest energy levels first.
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What do all the elements in the same group of the periodic table have?
The same number of electrons in their highest energy level (outer shell).
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What is each electron in an atom in?
An energy level.
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How can energy levels be represented?
As shells, with electrons in the lowest energy level closest to the nucleus.
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How many electrons can the lowest energy level or first shell hold?
Two electrons.
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How many electrons can energy levels after the lowest energy level hold?
Eight electrons.
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What energy levels do electrons occupy?
The lowest possible energy levels.
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What is the electronic structure of neon?
Neon has 10 electrons therefore has the electronic structure 2,8.
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What is the electronic structure of sodium?
Sodium has 11 electrons therefore has the electronic structure 2,8,1.
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What do Group 1 elements lithium, sodium and potassium have in common?
They all have one electron in their highest energy level. They react quickly with water and with oxygen.
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Why are nitrogen and phosphorus both in Group 5 in the periodic table?
Both have 5 electrons in their highest energy level (outer shell).
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**YOU SHOULD BE ABLE TO WORK OUT THE NUMBERS OF PROTONS, NEUTRONS AND ELECTRONS FOR ANY ATOM FROM ITS ATOMIC NUMBER AND MASS NUMBER***
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Card 2

Front

Where are electrons in atoms?

Back

In energy level that can be represented by shells.

Card 3

Front

Where are electrons in the lowest energy levels located?

Back

Preview of the front of card 3

Card 4

Front

In which order do electrons occupy energy levels?

Back

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Card 5

Front

What do all the elements in the same group of the periodic table have?

Back

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