help please...?

Question

An atom has an electron notation that ends 2p6. Which atom is it?
A.helium, He
B.neon, Ne
C.argon, Ar
D.krypton, Kr


Element X has an electron notation that ends with 4s1. Which of the following describes this atom correctly?
A.stable nonmetal
B.stable metal
C.unstable metal
D.unstable nonmetal


Which of the following is a transition metal?
A.barium
B.magnesium
C.lead
D.copper


Atoms which usually become negative ions because they tend to pick up electrons in a reaction are called
A.alkali metals
B.transition metals
C.nonmetals
D.actinoids


What are metalloids?
A.metals
B.nonmetals
C.gases
D.something between a and b

Gold, Au, should have an electron notation that ends in 6s25d9. To become more stable, the electrons in reality rearrange themselves. How do they do it?
A.6s15d5
B.6s25d10
C.6s15d10

Answer 1

1) B. Neon is in the second row of the periodic table so its configuration is 2s2, 2p6.

2) C. "Stable" and "unstable" are pretty vague terms, but the atoms with one S electron include sodium and potassium, both of which react explosively with air and/or water.

3) B. You just have to look at the periodic table to figure this one out--transition metals are in that long, narrow part in the middle of the periodic table.

4) C or D. I never heard of an actinoid, so I don't know if it's right or not. Most nonmetals do tend to pick up negative charges, but I don't know if they all do. I know it's not transition metals or alkali metals because they pick up positive charges.

5) D. A metalloid has both metallic and nonmetallic characteristics.

6) C. Atoms with unfilled d-shells commonly rearrange themselves by pulling electrons out of the s-shell and into the d-shell until either they get a full or half-full d-shell or they run out of s-electrons.

Answer 2

I am also taking Chemistry in ciollege. I found out that it is best to figure out electron configurations by looking at the trends of Periodic table, for example, where the s,p, d, and f orbitals are located and the period and group #s. This will be better than memorization.

#1) B. Neon (you are forgetting the 2s2 orbital...it should be 2s2 2p6)

#2) C. Unstable metal (because it is in group 1-A...it needs to lose 1 electron with a non-metal for stability by filling the valance shell)

#3) D. Copper (it is in group 1B in periodic)

#4) C. Non-metals (Groups 4A to 7A, which are non-metals, gain electrons)

#5). D. Something between metals and non-metals (this is what is used to make computer chips)

#6) C. 6s1 5d10 (all the s and p orbitals are your valence shells that lose or gain electrons normally)

Remember......It is best to follow the "patterns" of the periodic table by understanding the periods, group #s, and s,p,d, and f orbitals in terms of where they are located.

GOOD LUCK!!!

Answer 3

Sweetheart, these are pretty basic chemistry questions. If you plan to pass this class, you had better buckle down and study and learn the basics or I am afraid you are in for a horrible time.
I am not trying to be condescending or patronizing, but the sooner you figure these things out for yourself, the better. If you are lost this early in the class, you are really going to stay lost. GET YOUR TEXTBOOK OUT & STUDY INSTEAD OF SURFING THE NET!!!Just a word of advice!

Answer 4

B, C, D, C, D, C