1. Unit 2 Test Clicker Review

2. How does ionization energy trend within a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant

3. Which element has the smallest atomic radius?
A. Mg
B. P
C. Ca
D. Cl 

4. How does shielding trend across a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant 

5. What is the electron configuration of Phosphorus?
A. 1s22s22p63s23p64s2
B. 1s22s22p63s23p3
C. 1s22s22p63s23p63d3
D. 1s22s22p63s23p63d34s2 

6. Which block are the alkali metals in?
A. s block
B. p block
C. d block
D. f block

7. Which block are the transition metals in?
A. s block
B. p block
C. d block
D. f block 

8. Which block are the inner transition metals in?
A. s block
B. p block
C. d block
D. f block 

9. Which block are the noble gases in?
A. s block
B. p block
C. d block
D. f block 

10. The atomic number is always equal to the number of
A. electrons
B. neutrons
C. protons and electrons
D. protons 

11. Nitrogen- 16 has ___ neutrons and ___ protons
A. 9,7
B. 7,9
C. 16,7
D. 7,16

12. A neutral atom of an element has the same number of ____ as protons.
A. neutrons
B. electrons
C. neutrons and electrons
D. particles 

13. Dalton speculated that atoms of the same element are _____________ to one another.
A. identical
B. larger
C. smaller
D. different

14. Isotopes of an element differ in the number of
A. electrons
B. protons
C. neutrons
D. alpha particles 

15. Calculate the average atomic mass of a sample that is 80% Fe-55 and 20% Fe-56.
B. 55.8
C. 55.2
D. 55.0 

16. What particle has a negative charge and is 1/2000th the mass of a proton?
A. neutron
B. proton
C. electron
D. alpha particle 

17. How does electronegativity trend down a group?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant 

18. How does electronegativity trend across a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant

19. What did J.J. Thompson discover that were later called electrons?
A. positive particles he called corpuscles
B. negative particles he called corpuscles
C. neutral particles he called corpuscles
D. negative particles he called neutrons 

20.  Groups 1A-7A are called A. transition elements
B. representative elements
C. alkali metals
D. noble gases 

21.  Group 3-12 are called A. transition elements
B. representative elements
C. alkali metals
D. noble gases

22. Groups 3A-7A have incomplete __ sublevels.
A. s
B. p
C. d
D. f 

23. Transition metals have incomplete __ sublevels
A. s
B. p
C. d
D. f 

24. Horizontal rows are called ___ and vertical columns are called ___ on the periodic table.
A. periods, groups
B. groups, periods
C. transition, representative
D. representative, transition

25. Noble gases are ___ because they have ___ outer energy levels.
A. reactive, filled
B. inert, partially filled
C. inert, filled
D. reactive, partially filled 

26. Which of these has the highest electronegativity?
A. Be
B. N
C. Ne
D. Li 

27. Which of the following has the highest electronegativity?
A. O
B. S
C. Cs
D. Fr

28. Noble gases are in group
A. 1A
B. 7A
C. 2A
D. 8A 

29. Alkaline Earth Metals are in group
A. 1A
B. 7A
C. 2A
D. 6A 

30. Alkali metals are in group
A. 1A
B. 7A
C. 3A
D. 6A

31. 80% of the periodic table is
A. non-metals
B. transition elements
C. metals
D. solid 

32. In general, ___ are on the left side of the metalloid “stair-step” and ___ are on the right side of the metalloid “stair-step”. 
A. metals, nonmetals
B. metalloids, gases
C. gases, solids
D. p orbitals, s orbitals

33. Which noble gas would be used to write a noble gas configuration for magnesium?
A. Ne
B. Ar
C. Kr
D. Xe

34. Elements in the same group have the same number of
A. neutrons in highest occupied energy level
B. protons in the highest occupied energy level
C. alpha particles in the highest occupied energy level
D. electrons in the highest occupied energy level 

35.  What is Hund’s Rule? A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

36. What is the Pauli Exclusion Principle?
A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

37. What is the Aufbau Principle?
A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

38. Make sure you know orbital notation and can recognize if Hund’s Rule, Pauli Exclusion Principle or the Aufbau Principle is not followed!!