Transcript Slide 1

P. 208 – 58
Write electron configurations for the 2+ cations:
a. Fe
b. Co
c. Ni
P. 208 – 59
Write electron configurations for the 3+ cations:
a. Chromium
b. Manganese
c. Iron
P. 208 – 66
• If ionic compounds are composed of charged
particles (ions), why isn’t every ionic compound
either positively or negatively charged?
P. 196 – 12
• Use electron dot structures to determine formulas
of the ionic compounds formed when
a. Potassium reacts with iodine
b. Aluminum reacts with oxygen
P. 196-13
• What is the formula of the ionic compound
composed of calcium cations and chloride anions?
P. 199 – 22
Why do ionic compounds conduct electricity when
they are melted or dissolved in water?
P. 203 – 23
How do chemists model the valence electrons in
metal atoms?
P. 203 – 27
Why is it possible to bend metals but not ionic
crystals?
P. 207 – 46
Most ionic substances are brittle. Why?
47 – Explain why molten MgCl2 does conduct an
electric current although crystalline MgCl2 does
not?
48 – Explain briefly why metals are good conductors
of electricity.
51 – Explain why the properties of all steels are not
identical.
P. 203 – 25
Why are alloys more useful than pure metals?