Group 2
Quiz by Horia
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- Q1
What is the name of the group 2 metals?
Alkaline Earth Metals
Alkali metals
30s - Q2
Define metal
A substance formed from a regular lattice consisting of positively-charged metal ions surrounded by a sea of delocalized electrons and held together by the attraction between them (metallic bonds).
A substance formed from a regular lattice consisting of positively-charged metal atoms surrounded by a sea of delocalized electrons and held together by the attraction between them (metallic bonds).
30s - Q3
Write the electronic configuration of Ca2+
1s22s22p63s23p5
1s22s22p63s24s2
1s22s22p63s23p6
1s22s2
30s - Q4
Write the electronic configuration of Be
1s22s22p63s23p6
1s22s22p63s23p64s2
1s22s22p63s2
1s22s2
30s - Q5
Write the electronic configuration of Mg
1s22s2
1s22s22p63s2
1s22s22p63s23p64s2
1s22s22p63s23p6
30s - Q6
Write the electronic configuration of Ca
1s22s2
1s22s22p63s2
1s22s22p63s23p6
1s22s22p63s23p64s2
30s - Q7
Define atomic radius
Half the shortest internuclear distance found in the structure of an element. (Other values often used to represent the atomic radius are covalent radius, van der Waals radius and metallic radius.)
Half the shortest intermolecular distance found in the structure of an element. (Other values often used to represent the atomic radius are covalent radius, van der Waals radius and metallic radius.)
30s - Q8
State the trend in melting points down group 2
increases
decreases with Mg being an exception
decreases
30s - Q9
State the trend in atomic radius down group 2
increases
decreases
30s - Q10
Explain the trend in melting points down group 2
Increased shielding, there is a weaker attraction between the outer electrons and the nucleus (so there is less pull)
Atomic radius increases, shielding increases, the attraction between the positively charged ion and the delocalised electrons is weaker
Increased shielding, there is a weaker attraction between the outer electrons and the nucleus (so there is less pull).
30s - Q11
Explain the trend in atomic radius down group 2
Increased shielding, there is a weaker attraction between the outer electrons and the nucleus (so there is less pull).
Atomic radius increases, shielding increases, the attraction between the positively charged ion and the delocalised electrons is weaker
30s - Q12
Which group 2 metal has the lowest melting point?
Barium
Magnesium
30s - Q13
Explain the trend in first and second ionisation energies down the group
Increases, the atomic radius increases , shielding increases, therefore there is a weaker attraction between the positively charged nucleus and valence electron and this outweighs the increase in nuclear charge
Decreases, the atomic radius increases , shielding increases, therefore there is a weaker attraction between the positively charged nucleus and valence electron and this outweighs the increase in nuclear charge
30s - Q14
Explain the trend in reactivity down the group
Reactivity increases down the group as group 2 metals lose 2 electrons when they react. This is equivalent to the 1st + 2nd ionisation energy of that element. These values increase down the group due to the increase in shielding and atomic radius which outweigh the increased nuclear charge.
Reactivity increases down the group as group 2 metals lose 2 electrons when they react. This is equivalent to the 1st + 2nd ionisation energy of that element. These values decrease down the group due to the increase in shielding and atomic radius which outweigh the increased nuclear charge.
30s - Q15
Write the general equation for a group 2 metal reacting with water
M(s) + 2H2O(l) --> MO +H2(g)
M(s) + 2H2O(l) --> M(OH)2 +H2(g)
30s