11

Periodic Table Reference Table: S, Periodic Table

1. Dmitri Ivanovich Mendeleev arranged the elements in the periodic table by using the atomic mass.

2. Henry Moseley arranged the elements in the

periodic table by using the atomic number. 3. Periodic law: there is a periodic pattern in

chemical and physical properties of the elements in the periodic table. This is called Periodicity.

4. Periods: rows in the periodic table. Elements

in the same period fill up the SAME energy levels.

5. Groups: columns in the periodic table.

Elements in the same group have the same number of valence electrons, and similar chemical properties.

6. Elements are classified in 3 categories.

a. Metals: left of staircase b. Nonmetals: right of staircase c. Metalloids: touching the staircase:

B, Si, Ge, As, Sb, and Te except: aluminum (Al).

7. Properties of metals and nonmetals

PROPERTIES METALS

NONMETALS

Luster Yes No Malleable Yes No

Ductile Yes No Brittle No Yes

Conduct electricity Yes No

Conduct heat Yes No Electrons Lose Gain Ionization

energy Low High

Electronegativity Low High

Phase of matter Solid & liquid

Solid, liquid, & gas

Ions Positive Negative

8. Group 1 or Alkali Metals:

• form +1 ions, very active • found in nature as a compound: NaCl • Francium (Fr) is the most active element • forms strongest bases:

2 Na(s) + 2 H2O (l) à 2 NaOH(aq) + H2 (g) 9. Group 2 or Alkaline Earth Metals:

• form +2 ions • very active • found in nature as a compound.

10. Transition Elements (groups 3-12):

• have multiple oxidation states • appear colored, both in solid compounds

and in solution.

Example: CuSO4 (aq) CuSO4 (s)

11. Group 17 or Halogens: • form -1 ions; contains elements in three

phases of matter. F and Cl are gases, Br is a liquid and I is a solid.

• Found in nature as a compound. • The most active nonmetal is Fluorine (F).

12. Group 18 or Noble gases:

• generally non-reactive. Kr and Xe can form some bonds in the laboratory.

13. Monatomic gases (one atom): Group 18 14. Diatomic molecules (two atoms):

H2, O2 ,N2 ,Cl2 ,Br2,I2 ,F2

15. Electronegativity: attraction for electrons.

See table S.

12

16. Ionization Energy: The energy needed to remove an electron from an atom or ion. See table S.

17. All periodic table trends are influenced by

three factors: a. Energy level b. Shielding effect c. Nuclear Charge

a) Energy Level:

as you go down in a group the energy levels increases.

b) Shielding Effect: Core electrons block valence electrons from the nuclear charge of the nucleus.

c) Nuclear Charge: More charge pulls electrons in closer.

18. Trends in a Period: See table S and Periodic Table.

a) Atomic radii:

è Period: Decrease

Atomic radii decrease as you go across a period since there is an increase of nuclear charge (number of protons), which pulls the electrons in closer, thereby shrinking the size of the atom.

ê Group: Increase

Atomic radii increase as you go down in a group, since there is an increase in energy levels (shells).

b) Electronegativity:

è Period: Increases

The electrons increase across the period and therefore feel the “pull” more strongly.

ê Group: Decreases

The electrons are farther from the nucleus and therefore are more “shielded” by inner electrons from the pull of the nucleus.

c) Ionization Energy: Increases è Period:

The electrons increase across the period and therefore feel the “pull” more strongly.

ê Group: Decreases

The electrons are farther from the nucleus and therefore are more “shielded” by inner electrons from the pull of the nucleus.

2

6.941 +1 3 Li 2-1

3

22.98977 +1

11Na 2-8-1

4

39.0983 +1 19K 2-8-8-1

5

85.4678 +1

37Rb 2-8-18-8-1

6

132.905 +1 55Cs 2-8-18-18-8-1

7

(223) +1

87Fr -18-32-18-8-1

13

19. Trends Table Trends Period Group Atomic radii decrease increase Electronegativity increases decreases Ionization Energy increases decreases Metallic Character decreases increases

19. Allotrope: • Some elements may exist in two or

more forms in the same phase. • Different physical and chemical

properties. • Different molecular form.

Example 1: carbon is found as a graphite, diamond, and buckminsterfullerene

Graphite

Diamond Buckminsterfullerene Example 2: ozone and oxygen Ozone: Oxygen:

shape; bent shape: linear

Physical Properties

Graphite Diamond

Hardness (Mohs Scale)

1-2 10

Color Black Colorless Electrical Conductivity

Good Poor

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ELECTRONEGATIVITY

  1                                   18    

 1  

H  2.2          

                           

He  -­‐-­‐    

  1   2                       13   14   15   16   17   18      2  

Li  1.0    

Be  1.6    

                    B  2.0    

C  2.6    

N  1.9    

O  3.4    

F  4.0    

 Ne  -­‐-­‐    

 2   Li  1.0  

Be  1.6  

                    B  2.0  

C  2.6  

N  3.0  

O  3.4  

F  4.0  

Ne  -­‐-­‐    

3   Na  0.9  

Mg  1.3  

 3  

 4  

 5  

 6  

 7  

 8  

 9  

 10  

 11  

 12  

Al  1.6    

Si  1.6    

P  2.2    

S  2.6    

Cl  3.2    

Ar  -­‐-­‐  

   4  

K  0.8  

Ca  1.0  

Sc  1.0  

Ti  1.5    

V  1.6  

Cr  1.7  

Mn  1.6  

Fe  1.8  

Co  1.9  

Ni  1.9  

Cu  1.9  

Zn  1.7  

Ga  1.8  

Ge  2.0  

As  2.2  

Se  2.6  

Br  3.0  

Kr  -­‐-­‐  

   5  

Rb  0.8  

Sr  1.0  

Y  1.2  

Zr  1.3  

Nb  1.6  

Mo  2.2  

Tc  2.1  

Ru  2.2    

Rh    2.3  

Pd  2.2  

Ag  1.9  

Cd  1.7  

In  1.8  

Sn  2.2    

Sb  2.1  

Te  2.1  

I  2.7  

Xe  -­‐-­‐  

   6  

Cs  0.8  

Ba  0.9    

La  1.1    

Hf  1.3    

Ta  1.5    

W  1.7    

Re  1.9    

Os  2.2    

Ir  2.2    

Pt  1.9    

Au  1.8    

Hg  1.9    

Tl  1.8    

Pb  1.8    

Bi  1.9    

Po  2.0    

At  2.2    

Rn  -­‐-­‐  

   7  

Fr  0.7  

Ra  0.9  

Ac  1.1    

Rf   Db    

Sg    

Bb   Hs    

Mt    

Ds    

Rg    

Cn    

Uut    

Uuq    

Uup    

Uuh    

Uus    

Uuo    

 

12

Ionization Energy

  1               18    

 1  

H  1312  

             

He  2372    

  1   2   13   14   15   16   17   18      2  

Li  1.0    

Be  1.6    

B  2.0    

C  2.6    

N  1.9    

O  3.4    

F  4.0    

 Ne  -­‐-­‐    

 2   Li  520.  

Be  900.  

B  801  

C  1086  

N  1402  

O  1314  

F  1681  

Ne  2081  

 3   Na  

520  Mg  738  

Al  578    

Si  787  

P  1012  

 

S  1000.  

 

Cl  1251  

Ar  1521  

   4  

K  419  

Ca  590  

Ga  579  

Ge  762  

As  944  

Se  941  

Br  1140.  

Kr  1351  

   5  

Rb  403  

Sr  549  

In  558  

Sn  709    

Sb  831  

Te  869  

I  1008  

Xe  1170.  

   6  

Cs  376  

Ba  503    

Tl  589    

Pb  716  

Bi  703    

Po  812    

At  2.2    

Rn  1037  

   7  

Fr  393  

Ra  509  

Uut    

Uuq    

Uup    

Uuh    

Uus    

Uuo    

 

13

Group 1: Alkali

Group 3-12: Transition Elements

Group 17: Halogens

Group 18: Noble Gases

Semimetals

‘

1 18 1 H

He

1 2 13 14 15 16 17 18 2 Li Be B C N O F

Ne

3 Na

Mg 3 4 5 6 7 8 9 10 11 12 Al Si P S Cl

Ar

4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br

Kr

5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I

Xe

6 Cs Ba La

Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At

Rn

7 Fr Ra Ac f Db Sg Bb Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo

14

Metals Nonmetals Noble Gases Semimetals

           

 1                                   18    

 1   H                                  

 He    

  1   2                       13   14   15   16   17   18      2   Li   Be                         B   C   N   O   F  

 Ne    

 3   Na   Mg   3   4   5   6   7   8   9   10   11   12   Al   Si   P   S   Cl  

 Ar    

 4   K   Ca   Sc   Ti   V   Cr   Mn   Fe   Co   Ni   Cu   Zn   Ga   Ge   As   Se   Br  

 Kr    

 5   Rb   Sr   Y   Zr   Nb   Mo   Tc   Ru   Rh   Pd   Ag   Cd   In   Sn   Sb   Te   I  

 Xe    

 6   Cs   Ba   La   Hf   Ta   W   Re   Os   Ir   Pt   Au   Hg   Tl   Pb   Bi   Po   At  

 Rn    

 7   Fr   Ra   Ac   Rf   Db   Sg   Bb   Hs   Mt   Ds   Rg   Cn   Uut   Uuq   Uup   Uuh   Uus   Uuo