Topic 1 - The Periodic Table Flashcards Preview

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Flashcards in Topic 1 - The Periodic Table Deck (13)
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1
Q

How did Mendeleev arrange the elements in his periodic table?

A
  • Elements arranged with increasing atomic masses.
  • Elements with similar properties put into groups (due to periodic trends in chemical properties).
  • Switched the position of some elements. Gaps left for undiscovered elements.
2
Q

How was Mendeleev able to predict the properties of new elements?

A
  • Mendeleev left gaps in his periodic table.
  • He used the properties of elements next to these gaps to predict the properties of undiscovered elements.
3
Q

Mendeleev’s table lacked some amount of accuracy in the way he’d ordered his elements. Why was this?

A
  • Isotopes were poorly understood at the time.
  • Protons and neutrons had not yet been discovered.
4
Q

How are elements arranged in the modern periodic table?

A
  • In order of increasing atomic number.
5
Q

Fill in the blank: ‘Elements in the same group (column) have similar _______ ______’

A

Chemical properties

6
Q

Why do elements in the same column have similar chemical properties?

A
  • Same number of outer shell electrons
  • Number of outer shell electrons determines how an atom reacts.
7
Q

What does the period (row) number tell you about all the elements in that period?

A
  • Elements in the same period have the same number of electron shells.
  • e.g. all elements in period 4 have 4 shells of electrons.
8
Q

What does group (column) number tell you about all the elements in that group?

A
  • All elements in the same group have the same number of outer electrons.
  • e.g. all elements in group 2 have 2 electrons in their outer shell
9
Q

On which side of the periodic table are the metals positioned?

A

Left hand side.

10
Q

What determines whether an element is a metal or non-metal?

A

Atomic structures of the elements.

11
Q

What is the maximum number of electrons allowed in each of the first 3 shells?

A
  • 1st shell: 2
  • 2nd shell: 8
  • 3rd shell: 8
12
Q

When are atoms most stable?

A

When they have full electron shells

13
Q

The atomic number of Na is 11. What is the electron configuration of Na?

A

2, 8, 1