Review Periodicity Test
Name:_____________________________Per.____
PERIODIC TABLE – KNOW THE TERMS
Mendeleev
KNOW THE FOLLOWING GROUPS LOCATION:
Modern Periodic Law
VALENCE ePeriod – properties, e- config
GROUP I A- Alkali Metals
Group (Family) – properties, e- config
GROUP II A – Alkaline Earth Metals
Regions of the Periodic Table – know general locations
GROUP VII A – Halogens

Metals

Nonmetals

Metalloids
GROUP VIII A – Noble Gases
Know: Lanthanide Series & Actinide Series
1. What are valence electrons?
a. What happens to the number of valence electrons as you look down a group (column)?
b. What are the inner core electrons?
c. The element calcium has how many valence electrons? The element phosphorus?
2. What is the shielding effect?
3. How do the energy levels affect the reactivity of elements as you go down a group on the periodic table?
4. What are the two most reactive groups on the periodic table? Explain
a. As the nuclear charge (positive charge of the nucleus) increases, how would this affect the chemical
reactivity?
5. What do valence electrons have to do with chemical and physical properties of elements in the same
group?
a. Bacteria discovered in California were found to have Arsenic based DNA. Humans have Nitrogen
based DNA. How is life supported by to very different elements, especially when arsenic is
poisonous to humans? (think how does this relate to periodic trends…)
6. The ease at which an atom gains electrons is called what? Is energy a product or reactant of this effect?
7. The ability of an atom to attract electrons that are tied up in a chemical bound is called what?
a) What is the most electronegative element on the periodic table?
8.
What is the difference between electron affinity and electronegativity?
Determine which of the following elements answer the questions.
Circle one of the two elements in each pair (FOR A TOTAL OF 4) with the largest atomic radius (atomic size).
1. C - F
2. Zr - Pd
3. O - Mg
4. Ar - Sb
Circle one of the two elements in each pair with the smallest atomic radius (atomic size).
5. O - S
6. Se - Te
7. Al - In
8. O - N
Circle one of the two elements in each pair with greatest ionization energy.
9. P - Cl
10. F - Br
11. Na - S
12. Be - O
Circle one of the two elements in each pair with the least ionization energy.
13 . Mg - Ca
14. Rb - Sn
15. C - F
16. Te - In
Circle one of the two elements in each pair with the lowest electronegativity.
17. F - N
18. Cs - Na
19. Be - Sr
20. Cl – I
Circle one of the two elements in each pair with the highest electronegativity.
21. P - Cl
22. Mg - Al
23. Al - B
24. B - N
Circle one of the two elements in each pair with the largest electron affinity.
25. F - N
26. Cs - Na
27. Be - Sr
28. Cl - I
Circle one of the two elements in each pair with the smallest electron affinity.
29. P - Cl
30. Na - Al
31. C - Si
32. O - N
9. Circle the element with the highest electronegativity:
a.) P, In, O
b.) Xe, He, N
c.) Na, Mg, Sr
Circle one of the two elements in each pair with the largest atomic radius (atomic size).
10. a) N - F
b. Si - Cl
c. Na - Mg
d. Mg - Ca
Circle one of the two elements in each pair with the smallest atomic radius (atomic size).
11. a) O - S
b) Cs - Na
c) Al - P
d) O - N
12. In each set of elements determine the element with the lowest ionization energy:
a.) Ne, O, N
b.) Rb, K, Na
c.) He, H, Sr