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Week 3 Quiz
  • 1. Explain why ionisation energy increases as you move across a row (period) in the periodic table:
  • 2. Explain what ionisation energy is?
  • 3. How many electrons does carbon have?
A) 12
B) 0
C) 10
D) 6
  • 4. How many electrons does Sodium have?
A) 6
B) 0
C) 11
D) 12
  • 5. How many electrons does Argon have?
A) 0
B) 20
C) 24
D) 18
  • 6. What are the four different types of orbitals?
A) I, II, III, IV
B) W, X, Y, Z
C) S, P, D, F
D) A, B, C, D
  • 7. The valence electrons in carbon are in which orbital?
A) P
B) S
C) D
D) F
  • 8. The valence electrons in Magnesium are in which orbital?
A) D
B) S
C) P
D) F
  • 9. How many electrons can go in a S orbital?
A) 6
B) 18
C) 8
D) 2
  • 10. How many electrons can go in a P orbital?
A) 18
B) 8
C) 6
D) 2
  • 11. What element does this configuration represent?
A) Carbon
B) Boron
C) Lithium
D) Nitrogen
  • 12. What element does this configuration represent?
A) Aluminium
B) Germanium
C) Carbon
D) Silicon
  • 13. True or False: Elements in the same group (column) of the periodic table have the same number of electrons in their valence shell
A) False
B) True
  • 14. Elements in group 2 have how many electrons in their valence shell?
A) 8
B) 0
C) 1
D) 2
  • 15. Elements in group 1 make what charge when they lose their valence electrons?
A) +2
B) +1
C) -1
D) -2
  • 16. What element does this configuration represent?
A) Magnesium
B) Lithium
C) Sodium
D) Neon
  • 17. How many electrons in the last shell (atomic orbital)?
A) 10
B) 12
C) 8
D) 2
  • 18. Would the first ionisation energy be high or low for this element?
  • 19. Which one represents a noble gas?
A) 1s2 2s2 2p5
B) 1s2 2s2
C) 1s2 2s2 2p6 3s2
D) 1s2 2s2 2p6
  • 20. Which one would have a VERY high ionisation energy?
A) 1s2 2s2 2p5
B) 1s2 2s2
C) 1s2 2s2 2p1
D) 1s2 2s2 2p6 3s2
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