Download Review Periodicity

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Circle the word or phrase that best completes the statements.
1. (Calcium, Arsenic ) has the larger atomic radii.
2. (Calcium, Barium) has the larger atomic radii.
3. Down a group, atomic radii generally (increases, decreases, remains the same) because the
number of shells is (increasing , decreasing, remaining the same) therefore the nuclear force is
decreasing)
4. Across a period, atomic radii (increases, decreases, remains the same) because the nuclear
force or the hold on the electrons is (increasing, decreasing, remaining the same).
5. (Ionization Energy, Electronegativity, Electron reflection) is the atoms attractions of electrons
within a chemical bond.
6. (Sulfur, Selenium (Se)) has a greater electronegativity because it has a greater nuclear foce
with less shielding effect.
7. (Boron, Oxygen) has a greater electronegativity because it has a greater nuclear force.
8. Down a group electronegativity (increases, decreases, remains the same) because the number
of ( energy levels, protons, valence electrons) is increasing therefore the shielding effect is
increasing.
10. Across a period electronegativity (increases, decreases, remains the same) because the
number of protons in the nucleus is increasing with the same number of shells increasing the
nuclear force.
11. When calcium forms a stable ion it will (loose, gain) electrons called a(n) (cation ,anion)
12. When lithium forms a stable ion the charge will be __________________.
13. When phosphorus forms a stable ion it will (llose, gain) electrons called a(n) ( cation, anion)
14. When sulfur forms a stable ion the charge will be _____________.
15. The potassium ion is (larger, smaller, the same size ) than the neutral atom. The reason why
is electrons were (gained, lost, shared) making the nuclear force increase, decrease, remain the
same)
16. The silicon ion is (larger, smaller, the same size) than the neutral atom. The reason why is
electrons were (gained, lost, shared) making the nuclear force (increase, decrease, remain the
same)
17. An element that would react similar to calcium in a reaction would be ____________.
18. AN element that would react similar to bromine in a reaction would be ____________.
19. If carbon and oxygen were bonded in a molecule to one another, which one would the
electrons spend more time with? ____________ why?__________________________
20. Using your diagonal rule please complete the following:
Element/ Ion
Symbol # E
Electron Configuration
1. Lithium
2. Ion of Lithium
3. Arsenic
4. Ion of Arsenic
21. Cindy is working in the lab trying to do reactions with neon gas. She is unsuccessful. Why?
22. If potassium reacts with water by bubbling and releasing hydrogen gas, what would you
expect the reaction of lithium to be like? Francium?
23. How does the size of a metal determine the reactivity of the atom? WHY
24. How does the size of a halogen determine the reactivity of the atom? WHY?
25. Identify the most electronegative element in each set.
a. F vs. C
Al vs. Cl
b. Cs vs. I
Ca vs. Cl
26 Identify the element with the lowest ionization in each set.
a. F vs. C
Al vs. Cl
b. Cs vs. I
Ca vs. Cl
27. Identify the largest element in each set.
a. F vs. Cl
I vs. Cl
b. Cs vs. I
Ba vs. Cl