Bohr’s Diagrams (energy levels)

Energy Levels

It takes more and more energy for you to climb the steps.

With each higher step, you are at a higher energy level. You know this to be true because if you jump off a higher step you will land with more force than a lower step.

You can not stand in midair between the steps

Your energy levels are fixed.

You are ether on a step or not on a step.

While you are standing on a step, you neither gain nor loose energy.

Energy is required for you to move up a step.

Energy is released when you move down a step.

Bohr Model of the Hydrogen Atom

•According to the model, the electron can be only at certain distances from the nucleus, and not in between the orbits.

•Just as the lowest energy level of the stairs is a ground level, we say the lowest energy state of an atom is its “ground state”

•When the electron is in the E1 orbit, it is in its ground state.

•Any higher orbits (E2, E3) is called an excited state.

Energy Levels & Electrons

Find what row your element is on in the periodic table and draw that many energy levels (rings).

Resources Chapter menu

What does neon look like?

s orbital

1st main energy level – 2nd main energy level –

2 electrons 8 electrons

Shell Model Electrons are filled in successive layers, from lower energy levels

to higher levels.

Inner-shell electrons are called core electrons.

Electrons at the highest occupied energy level are called valence electrons.

Valence electrons are responsible for almost

all chemical properties of an element.

Inner-shell (core) electrons or core electrons

Highest energy level electrons or outer level electrons

Draw Bohr diagrams for O, F, Ne, Na, Mg

How many valence electrons do each of the

atoms have?

1 2 3 4 5 6 7 8

valence

The last digit of the

group number tells

you the valence.

Nobel Gasses

How many electrons does neon have in the lowest energy level?

How many electrons does Ne have in the 2nd energy level ?

How many electrons does Ne have have in the highest energy level?

How many valence electrons does Ne have?

Eight, which is the number of e- at the highest

occupied level.

•Note that the outer energy level is full

with eight electrons.

The Octet Rule • Noble gas atoms are unreactive because their

electron configurations are especially stable. • Nobel gasses have an octet (8) of electrons

in their highest occupied energy levels. • Except He which has a duet (2) of electrons.

• The octet rule: Ions and chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet (8) of electrons in its highest occupied energy level.

Section 2 Covalent Bonding and Molecular Compounds Chapter 6

The Periodic Table Section 2

The Role of Electrons

〉Why do elements within a group of the periodic table have similar chemical properties?

〉The periodic trends in the periodic table are the result of electron arrangement.

The Role of Electrons, continued

• Valence electrons account for similar properties.

• An element’s location in the periodic table is related to electron arrangement. – Example: Lithium and

sodium, in Group 1, each have one valence electron.

Ion Formation

〉What happens to an atom that gains or loses electrons?

〉If an atom gains or loses electrons, it no longer

has an equal number of electrons and protons. Because the charges do not cancel completely, the atom has a net electric charge.

Metals (H is a non-metal)

Non-metals (includes the Nobel Gasses)

1 2 3 4 5 6 7 8

valence

Metals lose their valence electrons to become

positive ions (cations)

Non-metals (excluding the Noble Gases) gain electrons to get an octet to become negitive ions (anions)

The octet rule: Ions and chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet (8) of electrons in its highest occupied energy level.

+ 2 e-

Formulas of anions (negative ions) are written with the element’s symbol and a superscript “-” sign If the charge is -2, -3, -4, the number comes before the “-” sign Example, oxygen ion is written: O2-

Gain of e- = negitive ion

Example: Cl-

The most stable ion that each of these elements forms is the ion that has an octet of electrons (which is a Nobel gas config) in its highest occupied energy level (the outer level). In each case, each ion has the same e- config. as neon.

1+ 2+ 3+ 4- 3- 2- 1- 0

Stable Ion

Charge

How many e-

needed to get

an octet?

Chemical Bonding

Positive ions attracted to negative ions = electrical attraction

Electrons are shared by neutral elements

Visual Concepts

Click below to watch the Visual Concept.

Visual Concept

Ionic Bonding

Chapter 6

Ionic Compounds – The positive and negative charges must balance

Na+ + Cl- = 1+ , 1- NaCl Na+ S2- = 1+ & 2-, so we need 1

more positive charge Thus we need 2 Na+

Na+ + Na+ + S2- Na2S

Elements from opposite ends of the table usually form ionic compounds.

Metal + non-metal = ionic bond

Non-metal + non-metal = covalent bond

Except: Hydrogen + group 17 = ionic bond Noble gases usually don’t bond

Hydrogen is a non-metal

Metals (H is a non-metal but it Usually forms positive(1+) ion

1+, 2+

3+,4-,3-,2-,1-

1 2 3 4 5 6 7 8 # valence e

Stable ion charge

Metals lose e-, become

+ ions (cations)

Non-metals (excluding the Nobel Gasses) gain e-, become – ions (anions)

No ions

metals Non-metals

1, 2 3 , 4, 3, 2, 1, 0

Number of Bonds =

Metals = # valence e-

Non-metals = 8 minus number of

valence electrons

Electron-Dot Notation • To keep track of valence

electrons, it is helpful to use electron-dot notation.

• Electron-dot notation is an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol. The inner-shell electrons are not shown.

Formation of Ionic Bonds

• The sodium atom has one valence electrons and the chlorine atom has seven valence electrons.

• Atoms of sodium and other alkali metals easily lose one electron to form cations (positive ion).

• Atoms of chlorine and other halogens easily gain one electron to form anions (negative ion).

• Positive & negative ions attract & form an ionic bond.

Section 3 Ionic Bonding and Ionic Compounds Chapter 6

Ions form crystals made up of trillions of atoms.

Section 3 Ionic Bonding and Ionic Compounds Chapter 6

Covalent Bonding

• Non-metals form covalent bonds. • Atoms share valence electrons so that the highest

occupied (by electrons) energy level (rings) has an octet (8) of electrons.

• Exception: Hydrogen only can have a duet of electrons (2).

• Thus the atoms share a pair of electrons.

7 valence

electrons

6 valence

electrons

Hydrogen atom

1 valence

electrons

F2, fluorine

Electron Spin Quantum Number

ms = +1/2 ms = -1/2

Spinning electric charges

cause a magnetic moment

with two possible

orientations Quantum No.s

What does neon look like?

s orbital

Lewis Dot Structures

Lewis Structures

• Electron-dot notation can also be used to represent molecules.

• The pair of dots between the two symbols represents the shared electron pair of the hydrogen-hydrogen covalent bond. • For a molecule of fluorine, F2, the electron-dot

notations of two fluorine atoms are combined.

• The Lewis structures and the structural formulas for many molecules can be drawn if one knows the composition of the molecule and which atoms are bonded to each other.

• A single covalent bond, or single bond, is a covalent bond in which one pair of electrons is shared between two atoms.

Lewis Structures

Lewis Structures • The pair of dots representing a shared pair of

electrons in a covalent bond is often replaced by a long dash.

• example:

Multiple Covalent Bonds Atoms of some elements, especially carbon, nitrogen, and oxygen, can share more than one electron pair.

A double covalent bond, or simply a double bond, is a covalent bond produced by the sharing of two pairs of electrons between two atoms.

All four electrons in a double bond “belong” to both atoms

A triple covalent bond, or simply a triple bond, is a

covalent bond produced by the sharing of three pairs of electrons between two atoms.

Double and triple bonds are referred to as multiple bonds, or multiple covalent bonds.

How many bonds can carbon form?

Each lonely electron can form a bond

Cyclohexane hexane

Chemical Bonding

Cholesterol

Starch is poly glucose

glucose

starch

Section 4 The Structure of Matter DNA

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