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Periodic Table - Group 1 Elements

A knowledge of the periodic table is a vital part of GCSE Chemistry. In this quiz we look at the group 1 elements - the alkali metals.

After many years of work by many different scientists, the periodic table was devised. The scientist given most credit was a Russian, Dimitri Mendeleev (pronounced Men-dell-ay-ef). He made the leap of faith that there were still many elements to be discovered and left gaps where he thought they should be. The metals account for most of the elements and appear on the left hand side of the table. The elements are arranged in vertical groups that contain elements that have similar chemical and physical properties.

The first group of elements of the periodic table is is made up from the most reactive metals. They have a variety of uses, for example lithium is used to manufacture laptop, tablet and mobile phone batteries, sodium is used in street lighting, potassium in fertilisers and caesium for making extremely accurate 'atomic' clocks used by scientists.

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Group 1 metals all react with cold water, in some cases very violently indeed. The reaction produces hydrogen gas and the hydroxide of the metal, which is strongly alkaline, giving the group its alternative name, the alkali metals. The reactions are exothermic, in fact, the heat released during the reaction of potassium and water is sufficient to ignite the hydrogen gas given off. The periodic table is all about patterns; as you descend the group, the metals become more reactive.

The reason for this and other patterns is the electron configuration. Group 1 is so-called because each of the elements has a single outer electron. During chemical reactions, atoms will either gain electrons, lose electrons or share electrons in order to achieve the structure of the nearest noble gas. It is only the outer electrons that are involved. The options for the group one elements are to either gain seven electrons or lose one electron - the latter is easier and this is exactly what happens. Atoms are neutral, they have the same number of electrons as protons. Since the number of protons remains the same during reactions, this loss of an electron means after reacting, the group one metals end up as ions with one positive charge. The reason that they are more reactive as you go down the group is that the outer electron is further from the nucleus. This means that they are not held as tightly and can be more easily lost.

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  1. Group 1 metals react with non-metals forming what type of bond?
    One electron is transferred to a non-metal atom during the reaction
  2. Group 1 elements only form what type of ion?
    They all lose one electron to achieve the electron configuration of the nearest noble gas
  3. How many electrons are in the outer shell of group 1 elements?
    That is why their group is named 'group 1'
  4. What gas is given off when group 1 elements react with water?
    Hydrogen gas burns with a squeaky pop
  5. Which of the following is NOT a property of group 1 metals?
    These metals can easily be cut using a scalpel
  6. When a group 1 element reacts with water, a hydroxide is formed. What colour would Universal Indicator turn in this solution?
    This shows that an alkali has been formed
  7. What colour flame is seen when potassium reacts with water?
    This is the characteristic colour of the flame when sodium vapour ignites
  8. Group 1 elements are also known as...
    When they react with water they form strong alkalis
  9. The reactivity of group 1 elements increases down the group. This is because...
    It becomes easier because the attraction between the positive protons in the nucleus and the electrons in the outer shell becomes weaker as the distance becomes greater
  10. Choose the correct order from the top to bottom of group 1.
    The size of the atoms increases down the group

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