Atomic radius increases going down a group, more shells. Atomic radius decreases going across a
9.
period, greater effective nuclear charge pulling in.
Metals = 2 /3 of all the elements. Lose electrons and form positive ions that are smaller than the parent
10.
atom. Ductile, malleable, have luster, conduct heat and electricity, most are solids at room temp, except
H
g,
low ionizati on energy, low electronegativity.
Nonmetals in upper right of table. Gain electrons and form negative ions that are larger than the parent
11.
atom. Brittle, dull, nonconductors, high ionization energy, high electronegativity, form covalent bonds.
t2. Metals are losers! Judge the reactivity of metals by how easily they lose electrons. The best metals lose
electrons the easiest fwant low ionization energy). Metallic character increases down & decreases
across. Best, most active, metals = Cs & Fr.
13. Nonmetals are winners! Judge reactivity of nonmetals by how easily they gain electrons. Best
nonmetals gain electrons the easiest [want high electronegativity). Nonmetallic character increases
across & decreases down. Best nonmetal, most active, = l'.
14. Metalloids fsemi-metals] = have some metallic and some nonmetallic properties - touching the line
except my palAl, he's a metal
Group 1 0A) = alkali metals. Very reactive. l- valence electron. Oxides: Mz0, Halides: MX
15.
t6. Group 2 fllAJ - alkaline earth metals.
2 valence electrons. Oxides:
M0. Halides:
MXz.
Group 17 IVIIA) = halogens. 7 valence electrons. (at room temp, Fz and Clz are gases, Brz is a liquid, and
17.
Iz is a solidJ
Group 18 [VIIIA]: Noble gases. 8 valence electrons, very stable, monatomic molecules. No compounds
18.
have ever been formed with the three lightest noble gases, He, Ne, and Ar.
!9. Transition metals
=
multiple positive oxidation states and have colored ions falso colored solutions and
colored saltsJ,
20.
Diatomic Elements: H2,F2, N2, 02, Brz,Clz,Iz. Brz and Hg are liquids.
Periodic Table Questions
1. what is nuclear charge? : rw'<y
2.
What is effective nuclear charge?
3.
What is ionization energ!?
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in
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.f..1- e-f
5. What are the trends for atomic size, ionization
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p-Lt!"\r**
i,\Lcryl f.-,_i r4i ilole,r"t_a e.
4. What is electgg4egativity? nff-e
t,>Y
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; g ss p*
energy, & electro negativity in the Periodic Table?