Periodic Table Review 1.Parts of the Periodic Table 2.Introduction to the Periodic Table 3.Atomic...

Periodic Table Review

1. Parts of the Periodic Table

2. Introduction to the Periodic Table

3. Atomic Structure and the Periodic Table

4. Periodic Trends in Atomic Radius, Ionization Energy, and Electronegativity

5. Isotopes and Average Atomic Mass

The columns are called groups or families. Groups have similar physical and chemical properties and the same number of valence electrons.

Name the groups boxed in yellow, orange, green and blue.

Name the groups boxed in yellow, orange, green and blue. Alkali metals, Alkaline Earth metals, Halogens, and Noble Gases

The rows are called periods. The period number matches the principle energy level of the element. This will be the principle energy level of the valence electrons.

What is the principle energy level of Nickel, Ni?

What is the principle energy level of Nickel, Ni? 4—it is in the row numbered 4

Using the Periodic Table

Let’s use the periodic table to answer some questions about Silicon

How many protons does Silicon have?

How many protons does Silicon have? 14 protons = atomic number

How many electrons does neutral Silicon have?

How many protons does Silicon have? 14 protons = atomic number.

How many electrons does neutral Silicon have? 14 electrons (# electrons = # protons in neutral atoms)

How many neutrons does Silicon-30 have?



How many neutrons does Silicon-30 have? 16 neutrons. Silicon-30 is an isotope of Silicon. It has a mass number of 30. The mass number is protons + neutrons.




What is the atomic mass of Silicon?




What is the molar mass of Silicon? 28.0855 amu (this is the same as the atomic mass on the periodic table)




What is the molar mass of Silicon? 28.0855 grams/mole (this is the same as the atomic mass on the periodic table)

How many valence electrons does Silicon have?




What is the molar mass of Silicon? 28.0855 grams/mole (this is the same as the atomic mass on the periodic table)

How many valence electrons does Silicon have? 4 valence electrons. Look for electrons in the highest principle energy level.

An s orbital holds 2 electrons w/ opposite spins

Each p orbital holds 2e- with opposite spins

Each d orbital holds 2e- with opposite spins

The s suborbitals fills

The orbitals and the periodic table

The p suborbitals fill


The d suborbitals fill


Valence electron configuration and the periodic table

All group 3a elements have the valance electron configuration ns2np1 and 3 valence electrons


All group 5a elements have the valance electron configuration ns2np3 and 5 valance electrons.


What is the valence configuration of the halogens?

Chemistry SOL Review—Atomic Structure


What is the valence configuration of the halogens? ns2np5.

Periodic Trends in Atomic Radius, Ionization Energy, and Electronegativity.

Atomic Radius: Half the distance between two atoms nuclei when they are bonded.

Ionization Energy: The energy needed to remove an electron from an atom.

Electronegativity: The tendency of an atom to attract electrons to itself when chemically combined with another element.

Atomic Radius: Half the distance between two atoms nuclei when they are bonded.

1 2 13 14 15 16 17 18

First Ionization Energy: The energy needed to remove an electron from an atom.

Ionization energy increases as you move to higher number groups. Group 8a has the highest ionization energy.

Ionization energy decreases as you move down the periodic table.

First Ionization Energy: The energy needed to remove an electron from an atom.

Electronegativity: The tendency of an atom to attract electrons to itself when chemically combined with another element.

The halogen group has the highest electronegativity of the families. The first period has the highest electronegativity. Noble gases do not have electronegativity as the valence shell is already full.

Anions, Cations, and Electron Configuration

Cations form by losing valance electrons to achieve a stable outer energy level.

Chemistry SOL Review—Atomic Structure


Cations form by losing valance electrons to achieve a stable outer energy level.

So Li loses the 2s1 electron to form Li+1.

Mg loses both 3s2 electrons to form Mg+2

Al loses three electrons from 3s23p1 to form Al+3

Chemistry Review—Atomic Structure


Anions form by gaining valance electrons to achieve a stable outer energy level.

So F becomes F1- by gaining a 2p electron to have the new valance configuration 2s22p6. S becomes S2- by gaining two 2p electrons to have the new valance configuration 3s23p6. N becomes N3- by gaining three 2p electrons to have the new valance configuration 2s22p6.

126C 13

6C 14

6C

Isotopes: elements with the same number of protons, but a different number of neutrons.

Carbon-14 has ___ protons and ___ neutrons

126C 13

6C 14

6C


Carbon-14 has 6 protons and 8 neutrons

126C 13

6C 14

6C


You figure out the average atomic mass of a compound by using a weighted average of the mass number for each isotope.

Example: a sample contains 10% C-13, 60% C-12 and 40% C-14. The average atomic mass is

(0.10 x 13) + (0.60 x 12) + (0.30 x 14) = 12.7

Periodic Table Review 1.Parts of the Periodic Table 2.Introduction to the Periodic Table 3.Atomic...

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