Final Exam Review: Chm 1.2

Final Exam Review: Chm 1.3

Understand the physical and chemical properties of atoms based on their position on the Periodic Table.

Chm 1.3

• Chm.1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition).

• Chm.1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table.

• Chm.1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.

Chm.1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition).

Periods

Groups

Valence Electrons

The Periodic Table

Group- Up and Down

Main group elements in the same group have similar properties, the same number of valence electrons, and the same

Period- Left to Right

Reactivity increases as you go down within a group for metals and decreases for nonmetals.

Valence Electron Cheat Code!

Element Classification

Representative Elements(main group)- A groups or as groups 1, 2, 13-18.

Transition elements as B groups or as groups 3-12.

Chm.1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table.

Periodic Trends

Electron Configuration

Electronegativity

A measure of the ability of an atom to attract the electrons

Electronegativity is not measured in energy units, but is rather a relative scale

Increase L to R, this is due to an increase in nuclear charge

Electronegativities generally decrease from top to bottom within a group due to the larger atomic size.

Atomic Radius

One of the ways we can express the size of atoms is with the atomic radius.

Helps us understand why some molecules fit together and why other molecules have parts that get too crowded

The atomic radius is defined as one-half the distance between the nuclei of identical atoms that are bonded together.

Electron Configuration

Electron configuration notation simplifies the indication of where electrons are located in a specific atom.

Hunds Rule

Aufubau's Principle

Pauli Exclusion

Hunds Rule

Every orbital in a sublevel is singly occupied before any orbital is doubly occupied.

Aufbau Principle

electrons fill lower-energy atomic orbitals before filling higher-energy ones 

Pauli Exclusion Principle

States that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins

Metallic Character vs Non Metallic

Metallic character refers to the level of reactivity of a metal; Metals tend to lose electrons in chemical reactions. Metallic character increases as you go down a group

Nonmetals tend to gain electrons in chemical reactions and have a high attraction for electrons within a compound. The most reactive NM:upper right portion of the periodic table

Multiple Choice

How many electrons can the first energy level hold?

• 1
• 2
• 8
• 0

Multiple Choice

How many electrons does Si contain? (click to see image)

• 14
• 28
• 2
• 4

Multiple Choice

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

• Zinc
• Copper
• Nickel
• Germanium

Open Ended

An atom has the electron configuration of 1s₂2s₂2p₅. How many electrons are in that atom? What atom is it?

Chm.1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.

Ionization Energy

Ionization Energy

Ionization energy is the energy required to remove an electron from a specific atom

Moving from left to right across the periodic table, the ionization energy for an atom increases

Ionization energy decreases as we go down a group.