2) How are polar covalent bonds different from nonpolar covalent bonds? ... d) If both of these orbitals were to occur in the same energy level, which...
BONDING & ELECTRONS EXAM REVIEW #2 11-20-214 1) Define the following terms. a) Frequency. b) Wavelength c) Core electrons d) Orbital e) Energy Level f) Pauli Exclusion Principle g) Valence Electrons
h) Triple Bond i) Bond j) Polar Covalent Bond k) Nonpolar Covalent Bond l) Lewis Structure m) Bonding Pair .
2) How are polar covalent bonds different from nonpolar covalent bonds? 3) Answer each of the following related to the compound to the right. a. Describe how all 4 chlorines have a stable octet. b. Describe how carbon has a stable octet. c. Indicate on the paper the shared and unshared electrons. d. Draw the stick structure for the compound.
5. The questions below relate to the images above.(2 pts each) a) What type of orbital is on the left? b) What type of orbital is on the right? c) How many electrons can fit into each of these orbitals? d) If both of these orbitals were to occur in the same energy level, which would be higher in energy? 5) Which of the following ions have the same electron configuration as the noble gas neon? a) K+
b) Na+
b) Mg2+
d) O2-
7) A light wave has a frequency of 6.0x1014 waves/s. a. Is this a form of visible light? Explain. b. Find the wavelength of the light. c. Calculate the energy of the light.
e) S2-
f) Al3+
8) For each of the following elements state whether it’s a metal, metalloid or nonmetal: a) Neon ________ d) Calcium ________ f) Silicon __________
b) Potassium ___________ e) Arsenic ___________ g) Tungsten ____________
c) Iron ___________ e) Bromine _________ h) Boron __________
9) A light wave has a wavelength of 350nm.
a. Is this a form of visible light? Explain. b. Find the frequency of the light. c. Calculate the energy of the light. 10) Neon has more electrons and protons than nitrogen, but has a smaller atomic radius. Explain why neon has a smaller radius. 11) Explain why potassium has a larger atomic radius than sodium. 12) As atomic radius gets smaller, in general ionization energy gets ______________. 13) The ionization energy is greater for neon than nitrogen. Explain this difference. 14) For each of the following molecules, draw the Lewis structure. a) ClF e) C2H6 h) BCl3
b) C2H4 f) P2 i) O2
c) BeH2 g) H2S j) Cl2
d) Br2 h) HCN k) Br2
15) Show how the following pairs of elements ionically bond. You must show the dot symbols and all ions formed. a) Calcium and Chlorine b) Sodium and Chlorine c) Barium and Nitrogen d) Magnesium and Oxygen
d) Calcium and Sulfur h) Aluminum and Oxygen e) Boron and Fluorine i) Lithium and Selenium f) Francium and Oxygen j) Hydrogen and Chlorine g) Beryllium and Phosphorus
