1. How many electrons can an s subshell hold? 2 2. How many electrons can a p subshell hold? 6 3. How many electrons can a d subshell hold? 10 4. Which subshells are available in the first energy level? 5. Which subshells are available in the second en- ergy level? 6. Which subshells are availabl...
1 how many electrons can an s subshell hold 2 2 how many electrons can a p subshell hold 6 3 how many electrons can a d subshell hold 10 4 which subshells are available in the first energy le
BTEC Applied Science Unit 1
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1. How many electrons can an s subshell hold? 2
2. How many electrons can a p subshell hold? 6
3. How many electrons can a d subshell hold? 10
4. Which subshells are available in the first
energy level? s
5. Which subshells are available in the second
en- ergy level? s and p
6. Which subshells are available in the third
energy level? s, p and d
7. What is Hund's rule? (Think bus seats!) Every orbital in a
sub-
shell must be singly
filled with an
electron before any
one orbital can be
doubly occu- pied,
and all electrons in
singly occupied
orbitals have the
same spin.
8. Which elements do not fill the 4s subshell Copper and
before the 3d subshell? chromium
9. Define the term ionic bond The electrostatic
attrac- tion between
oppositely charged
ions
10. What is the charge of an ion from group 1? +1
11. What is the charge of an ion from group 2? +2
12. What is the charge of an ion from group 6? -2
1/
, BTEC Applied Science Unit 1
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What is the charge of an ion from group 7? -
1 14.
2/
, BTEC Applied Science Unit 1
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Explain how atoms of sodium react with Na loses its 2s1
atoms of chlorine elec- tron gaining
a +ve charge.
Cl gains an electron
in the 3p subshell
gaining a -ve
charge.
The opposite
charges attract to
15. Why do ionic bonds have such high form NaCl
melting points?
Each +ve ion is
sur- rounded by 6
-ve ions and vice
versa.
Strong electrostatic
at- traction in every
direc- tion.
Requires a large
16. State two factors that affect the strength of amount of energy
an ionic bond to break
Size of ion and
charge on ion
17. When can ionic substances conduct electricity? When molten or in
aqueous solution
18. Describe the properties of ionic compounds Conduct electricity
when molten or
aque- ous solution
High
melting/boiling
points
Usually soluble in
water
19. Define the term covalent bond A shared pair of
elec- trons
3/
, BTEC Applied Science Unit 1
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Which metals lose electrons
from the 4s Transition metals
sub- shell before the 3d subshell?
21. Why do metals have such high melting points? Strong force of
attrac-
tion between positive
4/
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