Valence electrons are ALL the electrons in the last energy level, including s and p electrons.
Atoms will either lose all valence electrons, if they have less than four, or they will gain electrons, if they have more than four, to achieve the full and stable electron configuration like the noble gases.
1.
a. Show the complete or long hand electron configuration for fluorine, F. b. How many valence electrons does fluorine have? c. Will fluorine tend to gain or lose electrons? d. What is the charge on the stable fluorine ion? Show the fluorine ion symbol with
charge. e. Show the stable electron configuration with long hand for fluorine ion. Which noble or inert gas is the stable fluorine ion like?
2.
a. Show the complete or long hand electron configuration for calcium, Ca. b. How many valence electrons does calcium have? c. Will calcium tend to gain or lose electrons? d. What is the charge on the stable calcium ion? Show the calcium ion symbol with
charge. e. Show the stable electron configuration with long hand for calcium ion. Which noble or inert gas is a stable calcium ion like?

3. a. Write the electron structures of lithium and oxygen atoms. b) After drawing the structures of these two atoms draw their ionic structure. c) Is it possible for O to get its full octet of valence electrons from a single Li atom? d) What is the formula of the substance formed from the reaction of
Li metal with O
2
gas? (Hint: Use the ion formulas and the answer to question c to answer this question.)
4. Look at the figure below. The horizontal line is an energy scale that is lowest to the left and highest to the right. The arrow shows the direction of energy from low to high energy. Please show where the visible spectrum, red color, violet color, ultraviolet light and infrared light regions are on the diagram. The vertical lines are boundaries between visible spectrum and ultraviolet or infrared light. Each vertical line represents one of two colors. Remember that color represents energy in the visible spectrum.

5. The Bohr model of the hydrogen atom says that all energy levels in the hydrogen atom can be predicted by the following equation:
E=-13.6eV/n 2 n=1, 2, 3, 4 and so forth and eV is a unit of energy.
The normal state is for the hydrogen atom to be in the n=1 energy level. a) The hydrogen atom has how much energy when n=1 _________ ? b) How about the energy of the hydrogen atom when n=an incredibly large number__________? c) What is the difference in energy between a and b__________? d) When the electron is raised to this very large n value it is freed from the nucleus of the hydrogen atom so the hydrogen atom now has a positive charge.
What is this positively charged atom called __________? e) The energy that causes this positively charged atom to form is the
___________energy of the hydrogen atom?
For an extra 6 points: a) a) What is the energy difference between levels n=3 and 2 for the hydrogen atom and b) is energy lost or gained when the electron goes from level 3 to level 2? You must show your calculation below to get any credit for a. b)