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Review
1. At maximum, an f-orbital can hold __________ electrons, a d-orbital can hold __________ electrons,
and a p-orbital can hold __________ electrons.
2. Which one of the following orbitals can only hold two electrons?
3. What is the correct electron configuration for a ground-state nitrogen atom?
4. The ground-state electron configuration of the element __________ is [Kr]5s24d5
1
5. The element that has a valence configuration of 4s is _________.
6. The energy level of the first d-orbital is __________.
7. There are __________ orbitals in the second level.
8. The second energy level in the ground-state of a neutral atom of argon contains __________ electrons.
9. All of the __________ have a valence electron configuration ns1, where “n” is any number.
10. The largest energy level in the ground-state electron configuration of iodine is:
11. Elements in the modern version of the periodic table are arranged in order of increasing:
12. What is the atomic number of a neutral atom which has 51 neutrons and 40 electrons?
31 3
13. How many electrons does the ion 15
P contain?
14. The only noble gas that does not have the ns2np6 valence electron configuration is __________.
15. Which ions/atom have the same number of electrons?
I.
S2–
II. Cl–
III. Ne
16. What is the electron configuration for a Mg2+ ion?
17. Deduce the numbers of protons and electrons in the K+ ion.
18. An element is in group 4 and period 3 of the periodic table. How many electrons are in the highest
occupied energy level of an atom of this element?
19.
20.
21.
22.
How many protons, neutrons and electrons are present in each neutral atom of 31P?
Chlorine is much more apt to exist as an anion (negative ion) than sodium. This is because:
Sodium is much more apt to exist as a cation (positive ion) than chlorine. This is because:
What is the order of increasing energy of the orbitals within a single energy level?
Trends
23. Give the correct order for increasing atomic radius for Mg, Na, P, Si and Ar.
24. In which orbital does an electron in a phosphorus atom experience the greatest shielding?
25. The first ionization energies of the elements __________ as you go from left to right across a period of
the periodic table, and __________ as you go from the bottom to the top of a group in the table.
26. In general, as you go across a period in the periodic table from left to right:
(1) the atomic radius __________;
(2) the first ionization energy __________.
27. The atomic radii of the alkali metals increase down a group due to:
28. Which group on the periodic table has the lowest first ionization energies?
29. Which trend generally decreases across period 3?
30. Which trend increases down group 1?
31. Explain why the first ionization energy of magnesium is higher than that of sodium.
32. The relative atomic mass of naturally occurring copper is 63.55. Calculate the abundances of 63Cu
and 65Cu in naturally occurring copper.