Unit 4 Honors Chemistry Station Review
Station 1: Electron Configuration
1. Write the noble gas and standard form configuration for silver.
1s22s22p63s23p64s23d104p65s24d9
&
[Kr]5s24d9
2. Which element is [Xe] 6s25d5
Re
3. What period is [Xe] 6s25d5 in?
Period 6
4. What group is [Xe] 6s25d5 in? What is its name? Group 7b, Transition Metals
Station 2: Periodic Table Groups & Periods
1. Why is Krypton “perfect”? Complete valence shell (8 valence electrons) makes it stable
2. What do Ca, Ga, As, & Se all have in common? 4th period, 4 electron shells
3. What do Be, Ca, & Ba all have in common? 2nd group, 2 valence e-, Alkaline Earth Metals
4. What are valence electrons and how can you tell how many each element has (s & p
orbitals only!)? Outermost shell electrons, important for chemical bonding, determined
by group # (group 1a has 1, group 3a has 3, group 7a has 7 etc)
Unit 4 Honors Chemistry Station Review
Station 3: Coulombic Force, Ionization Energy, Electronegativity
1. Define coulombic force, ionization energy, and electronegativity.
Coulombic force ( attraction between protons and e-)
Ionization energy (energy it takes to “remove” 1 e-; forms a cation (+ charged ion) in a
covalent or ionic bond)
Electronegativity (e- affinity; determines how e- are shared in bonding)
2. Why do all three trends increase in energy as you go from L -> R across a period? Add P+
3. Why do all three trends increase in energy as you go UP a group? Decreasing radius
4. List these in order of increasing reactivity & explain your reasoning: He, Sr, Fr, P, Ga
(He, P, Ga, Sr, Fr)  lower Coulombic force means higher reactivity
Station 4: Metals, Non-metals, Metalloids
1. What is the BEST test to check for a metal? Conductivity (electricity)
2. List the metalloids. How can you tell where they are? B, Si, Ge, As, Sb, Te, Po
3. On which side of the stair-step line are the metals? Non-metals? L (metals), R (NM)
4. H and Al are exceptions. Which of the three subgroups do they fall into? H(NM), Al (M)
5. What are properties of metals? Non-metals? Metalloids?
M- ductile, shiny, strong, malleable, high density, solids at RT (except Hg), good
conductors
NM – brittle, weak, low density, poor conductors
Md- stronger than NM but less ductile than metals, somewhat conductive, etc
Unit 4 Honors Chemistry Station Review
Station 5: Atomic Radius
1. Define atomic radius. Distance from nucleus to outermost electrons
2. What is the trend in atomic radius across a period? Why? Decreases with increasing
coulombic force (e- are pulled closer to nucleus)
3. What is the trend going down a period? Why? Increases as you add shells
4. List these is order of smallest to largest size: F, K, O, B, Cs
(F, O, B, K, Cs)
Station 6: Periodic Table Groups/Families
1. What are the names of groups 1-8 (remember, this doesn’t include the transition
metals!) Alkali Metals, Alkali Earth Metals, Boron, Carbon, Oxygen, Halogen, Noble
Gases
2. What is the name of the d-block of elements? Transition Metals
3. What are characteristics of group 1 elements? 1 valence e-, highly reactive with water,
solids, does not include H, form cations (+ charged ions)
4. What are characteristics of group 8 elements? 8 valence e-, stable, non-reactive, gases,
no electronegativity