1. 5-1 R&R (Front) 6. Patterns of properties repeated every 8 elements
7. Proved periodic table correct when new elements were, in fact, discovered.
8. Properties of elements are periodic functions of their atomic number.
Mendeleev arranged by atomic mass.
1. c 2. a 3. b 4. d 5. -Similar properties - Average of the masses & densities of Be & Ca should give the approximate mass and density of Mg

2. 5-2 R&R name, symbol, atomic number, atomic mass
shiny, solid, condictive, malleable, ductile
distribution of electrons e b j h c g a j i k f m c d M SM NM
alkali metals
alkaline earth metals
halogens
noble gases

3. Atomic/Ionic Radius WS
1. Distance from center to outermost electron (size of atom) 2. Elements get smaller due to increased # of protons increasing nuclear pull 3. Elements get larger due to added energy levels 4. (a) chlorine (same row) (b) strontium (same column) (c) vanadium (same column) 5. (a) potassium (same row) (b) argon (same column) (c) cesium (same row) 6. Li, Be, C, F 7. B, Al, In

4. Atomic/Ionic Radius WS
1. Atom with charge due to gaining or losing electrons 2. lost; cation 3. gained; anion 4. smaller 5. larger 6. lose; positive 7. gain; negative 8. (a) Rb (b) I- 9. (a) Al+3 (b) S Review 1. periods 2. groups or families 3. 7; noble gas configurations

5. Periodic Trends Review
1. Periodic Law states that elements are a periodic function of their atomic #. This means that you see repeating patterns when elements are lined up by atomic #. This is important because it’s the basis of the modern periodic table!

6. 2. a. Fluorine – non-metal b. Germanium – metalloid c. Zinc – metal d
2. a. Fluorine – non-metal b. Germanium – metalloid c. Zinc – metal d. Phosphorous – non-metal e. Lithium – metal 3. a. Nobel gases – He, Ne, Ar, Kr, Xe, Rn b. Halogens – F, Cl, Br, I, At c. Alkali metals – Li, Na, K, Rb, Cs, Fr d. Alkaline Earth metals – Be, Mg, Ca, Sr, Ba, Ra

7. 4. Larger – added energy levels 5
4. Larger – added energy levels 5. Smaller – increased # of protons can pull the electrons in tighter. 6. a. Al or B b. S or O c. Br or Cl d. Na or Al e. O or F f. Mg or Ca

8. 7. Ionization Energy – the amount of energy needed to remove an electron 8. Positive = lose electrons  low I.E. requires less energy to remove an electron, so easier 9. Na = 1valence, so small I.E. (would rather lose 1 than gain 7). Mg = 2 valence, so I.E. wants to lose 2

9. 10. Lower – electrons further from the pull of the protons, so easier to remove 11. Increases – more protons to hold on (also, closer to 8) 12. a. Li or Be b. Na or K c. Cl or Si d. Ca or Ba e. P or Ar f. Li or K

10. 16. a. Ca or Ga b. Li or O c. Cl or S d. Br or As e. Ba or Sr
13. Electronegativity – the ability to attract an electron
14. Lower – electrons further from the pull of the protons, so not as able to attract
15. Increases – more protons to attract electron
16. a. Ca or Ga
b. Li or O
c. Cl or S
d. Br or As
e. Ba or Sr
f. O or S

11. 17. Electron Affinity– the energy gained when you gain an electron 18
17. Electron Affinity– the energy gained when you gain an electron 18. Lower – follows the trend of electronegativity 19. Increases – follows the trend of electronegativity

12. Study Guide 1.
a – Triads – groups of three elements with similar properties. Average mass/density of first & third about equals second
b – Octaves – patterns repeat every 8 elements
c – First periodic table – arranged by mass – left blank spaces
d – Periodic Law – rearranged periodic table based on atomic number

13. Study Guide 2.
a – Triads – groups of three elements with similar properties. Average mass/density of first & third about equals second
b – Octaves – patterns repeat every 8 elements
c – Element characteristics are periodic functions of their atomic number

14. “d” “p” “f” “s” Alkaline Earth Metals Alkali Metals Noble Gases
Nitrogen Group
Carbon Group
Oxygen Group
Boron Group
Halogens
“s”
“d”
“p”
Transition Metals
Lanthanides
“f”
Actinides
Inner Transition Metals

15. Study Guide
4 – He recognized places where the properties of the next element fit better if a blank space was left. This was where he predicted a new element would be discovered.
5 – group/family – vertical column on the periodic table
- period – horizontal row on the periodic table

16. Study Guide 6. a – [Ar] 4s23d2 b – [Kr] 5s24d8 c – [Xe] 6s24f6
d – [Kr] 5s24d105p4 7.
a – positive ion due to losing electrons
b – negative ion due to gaining electrons

17. Study Guide 8.
a – S-2
b – Ba+2
c – Ge±4
d – Al+3
e – Ne (no charge)

18. 9. a. Ca, Ge or Se b. C, Si or Sn 10 a. P or P-3 b. Sr or Sr+2 11. a
9. a. Ca, Ge or Se b. C, Si or Sn 10 a. P or P-3 b. Sr or Sr a. Na, Mg, or Si b. Na, Fr, or Rb

19. 12. a. Cs, Po or Tl b. At, F or I 13 a. Al, Si, or Mg b. Al, Tl, or In

20. Chapter 5 Practice Test 1. b 2. d 3. c 4. b 5. d 6. a 7. b 8. a 9. d

21. Chapter 5 Practice Test 11. F – Dobereiner 12 – (don’t worry about)
13. F - Moseley
14. T
15. F – non-metals
16. T
17. Na
18. N3-
19. Ca
20. O2-
21. Alkaline Earth metals – 4th period
22. Nitrogen group – 2nd period
23. XXX

22. Chapter 5 Practice Test 24. s,p,d,f – electron configuration
25. ionization energy – energy required to remove electron
electron affinity – energy gained when you gain an electrons
*opposites!
both higher for non-metals, lower for metals.
26. a. nonmetal (Cl)
b. Metal (Hg)
c. Non-metal (Se)

23. Chapter 5 Practice Test 27. He – outer shell only wants 2
28. H – not really a metal (doesn’t quite fit)
30. a. Lose 2
b. Lose 3
c. Gain 2
31. Se – oxygen group, period 4, nonmetal
32. decrease radius
increase ionization energy, electronegativity and electron affinity