GROUPS 1&2: ATOMIC AND PHYSICAL PROPERTIES

Quiz
•
Chemistry
•
11th Grade
•
Easy
Gwen Tan
Used 1+ times
FREE Resource
13 questions
Show all answers
1.
DRAG AND DROP QUESTION
30 sec • 2 pts
Explain why the atomic radii of the Group 2 elements increase as you go down the group. As you go down the group, you are adding (a) which take up more space. The (b) in the nucleus are exactly compensated for by the same number of extra shielding electrons, so there is no other effect to think about.
2.
DRAG AND DROP QUESTION
45 sec • 3 pts
Define the term first ionisation energy. The energy needed to remove (a) from each of (b) to make (c) .
3.
DRAG AND DROP QUESTION
1 min • 4 pts
Describe and explain how the first ionisation energy of Group 2 elements changes.
First ionisation energy (a) There are 3 considerations: (b) , the amount of shielding, and the distance of the electron from the nucleus.
As you go down the group, the extra charge on the nucleus is (c) by the inner electrons (shielding). The only factor affecting the ionisation energy is the distance from the nucleus. The (d) the outer electrons get, the less strongly they are attracted, and the lower the ionisation energy.
4.
DRAG AND DROP QUESTION
45 sec • 3 pts
The electronegativity of the elements falls as you go down the group. Explain what is meant by electronegativity.
Electronegativity is a measure of the tendency of (a) to (b) a (c) .
5.
DRAG AND DROP QUESTION
1 min • 4 pts
The most electronegative element in the group 2 is beryllium. Explain why beryllium is more electronegative than magnesium.
In both Be and Mg, the bonding pairs will feel a net pull of (a) – the number of protons minus the number of shielding electrons. But in the case of Be, the bonding pairs will be (b) to the nucleus than they are in Mg, because Be is a (c) atom than Mg. The (d) are more strongly attracted in Be and therefore the electronegativity of Be is greater than that of Mg.
Answer explanation
When the atoms form bonds there will be bonding pairs of electrons – each pair made of one from the Group 2 element and one from whatever it is bonding to. This applies just as well to the formation of ionic bonds as to covalent ones. In the case of the ionic bond, the bonding pair ends up very close indeed to the more electronegative atom in the bond - so close that we consider that the electron from the Group 2 metal has been transferred entirely to the other element.
6.
DRAG AND DROP QUESTION
45 sec • 4 pts
Explain why the single outer electron in both sodium (2,8,1) and potassium (2,8,8,1) feel the same net pull from the nucleus of +1. Sodium's nucleus has (a) , and there are (b) between the nucleus and the single outer electron. The outer electron therefore feels a net attraction of +1 from the nucleus. Potassium has (c) and (d) , also giving a net attraction of +1.
7.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
If both Na and K feel the same net pull from the nucleus, why is the potassium atom bigger than a sodium atom?
Potassium has an extra layer of electrons, and these take up space.
Sodium has an extra layer of electrons, and these take up space.
Potassium is more electronegative.
Potassium has bigger proton number.
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