. Use the periodic table to determine the element corresponding to each of the following electron configurations. a. [Ar]4s23d1 Express your answer as a chemical symbol. b. [Kr]5s2 Express your answer as a chemical symbol. 2. Arrange the following elements in order of decreasing atomic radius: Ba, Sb, Cl, Pb, and Se.

Two elements 1 and 2 are in the same row of the periodic table but not next to each other. Element 1 has a larger atomic radius than element 2, which of the following are most likely to be true about their relative ionization energies and why? O e a. I and IV b. II and IV c. III and VI d. I and V e. Il and V O b Od O a I. Element 1 has a larger ionization energy II. Element 2 has a larger ionization energy III. They both have the same ionization energy Because O c IV. electrons in element 1 are more strongly attracted to the nucleus V. electrons in element 2 are more strongly attracted to the nucleus VI. electrons are being removed from the same quantum shell

The first five ionization energies (IE, through IE) of a Period 2 element have the following pattern: kJ/mol IE₁ IE₂ IE3 IE4 IE5 Make a reasonable guess about which element this is. Enter its chemical symbol below. Ś

1. Write the electron configurations, both long (long) and Noble gas (NG), and orbital diagrams (OD) for: Be²+ long- Al As³- Fe NG - OD - long - NG - OD - long - NG - OD - long- NG - OD - Kau

Atomic radius 1. increases 2. decreases Because 1. the number of electrons increases 2. the mass increases 3. the relative attraction between the protons and the outer electrons increases ο ο ο ο ο ο O 2,1 O 1,2 2,3 2,2 1,1 from left to right across a row on the Periodic Table. O 1,3 #f #

Give the noble gas electron configurations and draw the valence orbital diagramsfor each of the following atoms or ions.a. Cub. V^2+c. Te^3-d. W

Write general outer electron configurations (nsxnpy) for groups 6A and 7A in the periodic table. The electron affinity of each group 7A element is more negative than that of each corresponding group 6A element. Use the electron configurations to explain why this is so.

10. Which of the following elements would have the greatest difference between the first and the second ionization energies? A) Ca B) Sr C) Na D) CI E) C

Give the indicated full or noble gas electron configuration Note: you can't do superscripts in questions answers, so format your answer without superscripts but with one space between each orbital. E.g. Li would be 1s2 2s1 instead of 1s22s The number in parentheses after the symbol is the element's atomic number. Full configuration: N (7) Full configuration: Si (14) Full configuration: Ti (22) Noble gas configuration: Ba (56) ( Noble gas configuration: Te (52) (99+ hp

Arrange the following groups of atoms in order of increasing first ionization energy.