Unit 4: Atomic Structure and Chemical Bonds

The electron structure of the atom

Why do atoms combine? An atom’s electrons travel in an area of

space around the nucleus called the electron cloud.

Scientists use a mathematical model that predicts where an electron is most likely to be, but cannot calculate the exact position of one electron.

Each element has a specific number of protons, neutrons, and electrons. The number of protons and electrons is the same for a neutral atom of a given element.

What an atom “really” looks like. How we will discuss atoms (useful model)

Electron Arrangement Some electrons are closer to the nucleus

than others. The different areas for an electron in an

atom are called energy levels. Each level represents a different amount of

energy. Each energy level can hold a maximum

number of electrons. The further away from the nucleus, the

more the energy level can hold.

Energy Level Number of electrons

1 2

2 8

3 18

4 32

Bohr Model We can create a model

of an atom just like Bohr thought they would look It’s not exactly how a

“real atom” looks, but it helps us to get a good idea of what is going on inside of an atom.

Creating a Bohr Model1. Calculate the number of protons,

neutrons, and electrons in the atom. 2. Write the number of protons and

neutrons in the middle of the model.3. Figure out how many electrons will go

on each level (remember, 1st level- 2 e-, 2nd level = 8 e-, 3rd level =18 e-, ect.)

4. Draw the electrons on the appropriate energy levels.

Bohr Model Examples Carbon

Bohr Model Examples Magnesium

Bohr Model Examples Chlorine

Energy Steps Electrons in the level closest to the

nucleus are in energy level 1. Have the lowest amount of energy.

Electrons farthest from the nucleus have the highest amount of energy. Easiest to remove.

Electron Configuration Atoms with a complete outer energy

level are stable. Want 8 electrons in the outer energy

level. Elements in the noble gases are stable,

because they have 8 electrons in their outer energy level.

Electron dot diagrams An electron dot diagram is the symbol for

the elements surrounded by as many dots as there are electrons in the outer energy level.

Only outer energy level electrons shown because they determine how the element can react.

Use electron dot diagrams to show how atoms form chemical bonds. The force that holds two atoms together.

Practice: Iodine:

Neon:

Sodium:

Practice: Magnesium:

Aluminum:

Phosphorus:

Bonding in elements

Substances Matter that has the same composition and

properties throughout is called a substance. When different elements combine through

bonding, they form new substances.

Ionic Bonds Ionic Bonds always form between a metal

and a nonmetal. Ion- an atom that is no longer neutral

because it has lost or gained an electron. Metals want to lose electrons to become

positive ions (cations) Nonmetals want to gain electrons to

become negative ions (anions) Cations (positively charged) and anions

(negatively charged) are strongly attracted to each other. This creates ionic bonds.

Forming Ions All ions want to have 8 valence

electrons. Atoms that have 1 , 2, or 3 valence

electrons will lose electrons from their outer most energy level, so that they are left with the next full layer on the outside.

Forming Ions All ions want to have 8 valence

electrons. Atoms that have 5, 6, or 7 electrons on

their outermost energy level will gain electrons to fill the outer energy level up to 8 electrons.

Example: Sodium wants to give away its one valence electron, chlorine wants to gain one valence electron, so they make an ionic bond.

Examples: What charge of ion will these atoms form? Together: Lithium Beryllium Boron Fluorine

On your own: Magnesium Potassium Sulfur Bromine

Drawing Ionic Bonds Lithium + Bromine

Lithium Bromide

Drawing ionic bonds Magnesium + Chlorine

Magnesium Chloride

Drawing Ionic Bonds Sodium + Sulfur

Sodium Sulfide

Covalent Bond Forms between two nonmetals. Both atoms involved in the bond want to

gain electrons. Instead of giving or taking electrons, the

two atoms share electrons. The shared electrons belong to both

atoms now. Atom will share as many electrons as they

need to gain. The neutral particle formed when atoms

share electrons is called a molecule.

Drawing Covalent Bonds 2 Hydrogen

Hydrogen GasTriangulum Galaxy

Drawing Covalent Bonds 2 Hydrogen + 1 Oxygen

Water (on a blade of grass)

Drawing Covalent Bonds Carbon + 2 Oxygen Atoms

Carbon DioxideEmissions from factory

Drawing Covalent Bonds Nitrogen + Nitrogen

Nitrogen Gas

Types of Covalent Bonds Double and triple bonds- when

an atom shares more than one electron with another atom. Two pairs of electrons shared-

double bond Three pairs of electrons shared-

triple bond Polar bond- a bond in which

electrons are shared unevenly. Some elements, like oxygen, hold

the electrons very close to them and rarely share with their partner.

Metallic Bonding Metal atoms bonded together form metallic bonds. Metals do not hold onto their outer electrons very

tightly. Instead, in a metallic bond, the electrons flow freely

amongst all metal ions in a pool or “sea” of electrons. Metallic bonding is why metals are malleable, ductile,

and conduct electricity.