1. What is the electron configuration of neutral phosphorous
What is the electron configuration of neutral phosphorous? 1s22s22p63s23p3
1s22s22p63s23p3
Phosphorous is located here

2. Atomic Trends
How does atomic radius change down a group in the periodic table?
It tends to increase.

3. Why is the radius of a positive ION always less than the radius of its NEUTRAL atom?
It gave away an electron, and the nucleus pulls the remaining electrons in closer.
Na neutral sodium
11 electrons
11 protons
Na 1+ sodium ion
10 electrons
11 protons

4. What term is used to describe an atom's tendency to attract electrons (selfish of electrons) to itself when it is chemically combined with another element?
electronegativity
Really greedy because they are so close to having 8 valence electrons.

5. The noble gases don’t want or do much
Which group of the periodic table has the highest electronegativity?
7A, the halogens
The noble gases don’t want or do much
More
greedy
for
electrons
More
greedy
for
electrons

6. Which of the following elements has the lowest electronegativity (selfishness of electrons)?
Choose the cation with the least valence electrons and the most amount of total electrons.
More
greedy
for
electrons
More
greedy
for
electrons

7. Electronegativity generally increases from left to right across a period.
More
greedy
for
electrons

8. Compared with the electronegativities of the elements at the left end of a particular period,
the electronegativities of the elements at the right side of that same period (ROW) tend to be higher.

9. Which of the following factors contributes to the relatively greater atomic size of the higher-atomic-number elements within a particular family of the periodic table?
More shielding of the outer electrons by the inner electrons

10. Groups (family or column)H
As we go down a group each atom has another energy level
More shielding
The outer electrons have greater freedom from the nucleus. Li Na K Rb

11. Which of the following increases with increasing atomic number (GOING DOWN) in Group 2A?
atomic radius…the electrons have more freedom to move outward because of shielding.

12. How does the shielding phenomenon affect the relative atomic sizes of elements in the same period (row)?
Shielding has no effect on relative atomic size within a period. Na Mg Al Si P S Cl Ar

13. The one that is furthest right.
Which of the following elements has the smallest atomic radius?

14. Atomic size generally decreases as you move from left to right across a period (row).

15. The energy required to remove an electron from a gaseous atom is called the ionization energy.
Na neutral sodium
11 electrons
11 protons
Na 1+ sodium ion
10 electrons
11 protons

16. When is an electron configuration particularly stable?
When its last principle energy level is a filled.

17. For Group 3A metals, which electron is the most difficult to remove from a neutral atom?
the fourth because it was meant to give away the three in the valence shell, but the fourth is going into an inner shell that was already stable.

18. Which of the following factors contributes to the huge ionization energy of the elements on the right side of a period in the periodic table?
greater number of protons in nuclei and the number of valence electrons is so close to the number 8
Don’t
want to
give away
electrons
Don’t
want to
give away
electrons

19. Which of the following elements has the smallest FIRST ionization energy?
The elements in the 1A column because they are so anxious to get rid of that one valence electron.
Don’t
want to
give away
electrons
Don’t
want to
give away
electrons

20. As you move from left to right across the second period (row) of the periodic table the ionization energy increases
Ionization energy increases because
they don’t want to give away electrons
Don’t
want to
give away
electrons

21. Ionization energy needed & Electronegativity
SIZE of atomic radius/diameter
SIZE of atomic radius/diameter

22. pick positive cations before negative anions.
Of the following atoms, which one has the smallest FIRST ionization energy?
pick positive cations before negative anions. +1 +1 +3 +2 +1 +3 +2 +1 +2 +1 +2

23. Which of the following elements, would ionically bind to sulfur?
metals bond with
non-metals for an ionic bond. +1 +1 +3 +2
Back to REVIEW
In document
form +1 +3 S +2 +1 +2 +1 +2