1. Unit 3 Review
Honors Chemistry

2. 2-Alkaline
Earth
Metals
1-Alkali
Metals
18- Noble Gases
17-Halogens
Transition Metals

3. High IE and EN Small atoms! High IE and EN Highest IE Highest EN
Lowest IE

4. Organized by increasing atomic number1 2 3 4 5 6 7

5. Atomic Radius Trends Smaller across period – higher nuclear charge
Bigger down-
More energy levels!

6. Metals (red – for review wksht)
Nonmetals (blue for review wksht)
Metalloids (green – for review worksheet)

7. 11) Have 1 valence electron ____________________
12) Have 8 valence electrons
____________________
12) Have 7 valence electrons
13) Have 2 valence electrons
Alkali metals – group 1
Noble Gases – group 18
Halogens – group 17
Alkaline Earth metals – Group 2

8. 14) The least reactive elements ____________________
15) The most reactive nonmetals (gases at room temperature)
16) The most reactive metals
17) Reacts readily with oxygen and water
18) Used to make coins and jewelry.
Noble Gases
Halogens
Alkali metals
Alkali Metals
Transition Metals

9. 19) Energy required to remove an electron from an atom
____________________
20) The ability of atom to attract electrons.
21) List 3 other elements that will have similar chemical properties to Nitrogen and explain why.
Ionization Energy
Electronegativity
Phosphorus, Arsenic and Antimony
Same group –gives them same # of valence electrons and ion charge, therefore similar reactivity!

10. 22. Circle the element in the pair has the larger ionization energy
22. Circle the element in the pair has the larger ionization energy. Explain why.
a. Li, N b. Kr, Ne c. Cs, Li
23. Explain the octet rule.
24. Circle the element in the pair is more electronegative. Explain Why?
a. K, As b. N, Sb c. Sr, Be
Smaller atoms – have less shielding – higher nuclear charge to hold on to its valence electrons!
Atoms will lose or gain electrons to have 8 valence electrons in their outer energy level.
Smaller atoms – less shielding – nucleus charge is stronger and can attract the electron more easily.

11. 25. Periodic law states that elements show a
a. repetition of their physical properties when arranged by increasing atomic radius.
b. repetition of their chemical properties when arranged by increasing atomic radius.
c. periodic repetition of their properties when arranged by increasing atomic number.
d. periodic repetition of their properties when arranged by increasing atomic mass.
26. Elements in the same group of the periodic table have the same:
a. number of valence electrons b. physical properties c. number of electrons
27. Which of the following is NOT true of an atom, other than Helium, obeying the octet rule?
a. obtains a full set of 8 valence electrons
b. acquires the valence electrons of a noble gas
c. possess 8 electrons in total
d. has a s2p6 valence configuration

12. a. atomic radius, ionization energy
28. Moving down the periodic table, which two atomic properties follow the same trend?
a. atomic radius, ionization energy
b. atomic radius, electronegativity
c. ionization energy, electronegativity
d. none of the above
Which will form a larger ionic radii than its’ parent atom?
a. cation (+ ion) b. anion (- ion)
Explain your choice!
Extra electrons cause repulsion and cloud spreads out – ion gets bigger!

13. 30) How many electrons does an atom of Oxygen have? _____
How many electrons does 0-2 have? _____
31) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why fluorine holds on to its electrons so well)
8 total, 6 valence electrons
10 total, 8 valence
NUCLEAR

14. 1s2 2s2 2p6 3s2 3p6 4s2 3d6
32) Which element is this for? ____________________-
33) In which period is this element found in?______ In which group #? _______
34) How many electrons are in this element’s 3rd energy level? _____
35) Re-write the electron configuration of this element if it became an ion with a +2 charge
Fe - Iron 4 8 14
1s2 2s2 2p6 3s2 3p6 3d6
It loses the 2 electrons in 4s
d-orbitals do not change!

15. 38) How many electrons can fit into 1 orbital? _____
36) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found.
37) How many orbitals are in each sublevel? a. S = ___ b. P = ___ c. d = ___ d. F = ____
38) How many electrons can fit into 1 orbital? _____
Cloud Shaped
Electron 1 3 5 7
2 electrons

16. 39) What do the quantum numbers tell us about an atomic orbital?
The probable location of an electron
The main energy level it is on.
The shape of the orbital (s, p, d or f) it is in.
The orientation of that orbital around the nucleus
The spin direction of the electron

17. 40) Is the following orbital notation for the 3rd and 4th energy levels of the element in #32 above correct? Explain
3s p s d
It is not correct, the 3d orbitals should have one in each orbital and then it should double up!

18. #40

19. 41) Identify the blocks where these groups are found –
a. Halogens = ____ block
b. Alkaline Earth Metals = _____ block
c. Alkali Metals = ______ block
d. Rare Earth Metals = ______ block
e. The Noble Gases = _____ block
f. The Transition Metals = _______ block p s s f p d

20. Photons and the Electromagnetic Spectrum
41) An electron that is closest to the nucleus possible (at the lowest energy level possible) is said to be in its ___________ _________________.
42) When an electron jumps up to a higher energy level and then falls back to its ground state a ___________ is released.
Ground State
Photon

21. Photons and the Electromagnetic Spectrum
43) The amount of energy released by an electron jumping from the 4th energy level back to its ground state at the 3rd energy level will always release a photon with a___________________________ (different-variable/specific-quantized) amount of energy.
44) The color spectra (types of colors produced) of a star can be used to identify the types of ______________ present in the star.
Elements