Chapter 6 Chapter 6 Chemical CompoundsChemical Compounds

Chapter 6 Chapter 6 Chemical CompoundsChemical Compounds

6-1 Ionic Bonding6-1 Ionic Bonding

Stable Electron Configurations

• When the highest occupied energy level of an atom is filled with electrons, the atom is ___________ and not likely to react

• Chemical properties of an element depend on the number of _________ electrons

Electron Dot Diagram• An ____________ is a model of an

atom in which each dot represents a _____________ electron

• The symbol is in the center represents the_________ and all the other electrons in the atom

Electron Dot Diagrams Group 1

Group 2

Group 3

Electron Dot DiagramsGroup 4

Group 5

Group 6

Electron Dot DiagramsGroup 7

Group 8

Ionic Bonds• Some elements achieve stable electron

configurations through the __________ of electrons between atoms.

• Ex Chlorine atom has________electron fewer than an argon atom

• Chlorine _________ a valence electron, it would have the same stable electron arrangement as _________

Formations of Ions• When an atom ______ or _________an

electron, the number of protons is no longer _________ to the number of electrons.

• An atom that has a net________ or ________ electric charge is called an_______.

• The charge on an ion is represented by a ______ or__________ sign

•Na:

•Cl:

•Na+1 sodium ion Cl-1 chloride ion [Ne] [Ar]

Anion verses cation• An ion with a __________ charge is

an ________ Ex: Cl-1

• An ion with a_________ charge is a __________ Ex: Na+1

Formation of Ionic Bonds

6-1 continued• When an anion and a cation are close

together, a chemical_________ forms• A __________ bond is the force that holds

atoms or ions together as a__________.• An _________ bond is the force that

holds cations and anions together• An ________ bond forms when electrons

are transferred from one atom to another

Ionization energy• The amount of energy used to

remove an_____ is called_________energy

• Ionization energy tends to_______ from left to right________ a period.

• They tend to_______ going down a_________

Ionic Compounds• A chemical ___________ is a notation

that shows what elements a compound contains and the_________ of the atoms or ions these elements in the compound.

• Ex: chemical formula =_________ (sodium chloride)

• Ex: MgCl2

Crystal Lattices• Solids whose particles are

arranged in a lattice structure are called___________

•Ionic bondingwithin a crystal lattice

•Covalent bondingforms a “molecule”

Properties of Ionic Compounds

• The properties of an ionic compound can be explained by the__________ attractions among ions within a crystal ________.

• Have _________ melting points• Ions with same charges (- and -) or (+

and +) __________ each other• Ions with the opposite charges (+ and -)

_________ each other.

6-2 Covalent Bonding• _________ bond is a chemical bond

in which two atoms_______ a pair of valence electrons

• When two atoms share one pair of electrons, the bond is called a _________ bond

Molecular Models• Electron Dot diagram of H2

Molecular Models• Structural formula of H2

Molecular Models• Space-filling model of H2

Molecular Models• Electron Cloud Model of H2

Molecules of Elements• A _______ is a neutral group of atoms

that are joined together by one or more covalent bonds

• The __________ between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond

• Diatomic means ________atoms

Lewis structure

Single bond: covalent bond producedby the sharing on ONE pair of electronsbetween 2 atoms

Multiple Covalent Bonds

•DOUBLE BOND

–sharing of________ pairs of electrons between 2 atoms

•TRIPLE BOND

–sharing of __________ pairs of electrons between 2 atoms

• Bond Energies:

• triple > double > single

…..triple bonds are stronger and shorter

Think Pair Share• You and your partner think of

situations that serve as analogies for ionic and covalent bonding.

Draw the Lewis structure for carbon

tetrachloride• CCl4• Total # of valence electrons:

– C: 1 x 4 e- = _______ e- – Cl: 4 x 7 e- = _______ e-

• Total # = ______ e-

or…..

Practice• Draw the Lewis structure of IBr

Beaker Breaker• Draw the Lewis structure showing

bonds for • HBr

• CH4

6-2 Continued• A ____________bond in which electrons are not

shared equally is called a _______ covalent bond.

• _________ – opposite in character, nature, or direction

• When atoms form a polar covalent bond, the atom with the __________ attraction for electrons has a partial __________ charge. The other atom has a partial _________ charge.

Polar and Nonpolar Molecules

• If a molecule has only______atoms, it will be _________

• When molecules have more than______atoms, the answer is not as obvious.

• The _______ of atoms in a molecule and its ________are factors that determine whether a molecule is_______ or ______

• See figure 12 page 168

Attraction between Molecules

• Attractions between polar molecules are _______ than attractions between __________ molecules

• Ex: water verses methane (CH4)• Methane = ________• Water = _______• Boiling point of water is _______

Practice• Complete Section 6-2 Review page

169 Questions 1-8

6-3 Naming Compounds and Writing Formulas

• Chemists use a system for naming compounds that is based on ________

• The chemical name for lime is calcium oxide and the chemical formula is ______

• ______ to_____ ratio of calcium ions to oxide ions in calcium oxide

Describing Ionic Compounds

• The name of an_______ compound must distinguish the compound from other ionic compounds containing the _______ elements.

• The formula of an ionic compound describes the ______ of the ions in the compound

Binary Ionic Compounds

• A compound made from only two elements is a _______ compound

• The names have a predictable pattern; the name of the________ followed by the name of the ______

• Name for the cation is the name of the_______ without any change

• Name of the anion used part of the name of the _________with the suffix “_______”

• Ex : NaCl = ____________

Metals with Multiple Ions

• The alkali metals, alkaline earth metals, and aluminum form ions with___________charges equal to the _______ number

• Ex: potassium = ______• : calcium = ______• : aluminum = _______

Transition Metals• When a metals forms more than one ion,

the name of the ion contains a_______ numeral to indicate the ______ on the ion

• Example Copper(I)oxide = Cu+1O-2

• The formula balanced equals _____• Copper (II) oxide = Cu+2O-2

• The formula balanced equals _______

Polyatomic Ions• What does the prefix “poly” mean?

• A covalently bonded group of atoms that has a positive or negative charge and acts as a unit is a___________

• See figure 19 on page 173

Practice• What are the names of these

binary ionic compounds:• LiCl • BaO

• Na3N

• PbSO4 use table on 173

Practice • The charge on a chloride ion in

AlCl3 is?

• Write the formulas for the following compounds:

• Copper(I)chloride• Copper(II)chloride

Homework/More Practice

• Name the following Binary compounds:

1. Na2S =

2. Li2O =

3. MgBr2 =

4. H2S =5. AlN =

Homework/More Practice

• Name the following using the Roman Numeral system

1. SnO =2. TiO =3. TiCl3 =4. CuCl =5. NiBr2=

6-3 continued Describing Molecular

Compounds• The name and formula of a

________ compound describes the ________ and ______ of atoms in a molecule of the compound

Naming Molecular Compounds

• Consists of two _________ in a compound• The name of the________element is

changed to end in the suffix “ide”• You use Greek _______ to describe how

many atoms of each element there is present (see handout)

• Ex: carbon dioxide = ______ or can be named as ________________, mono is usually not used for the first element

Writing Molecular Formulas

• Write the ________ for the elements in the order the elements appear in the name

• The _________ indicate the number of atoms of each element in the molecule

• Prefixes appear as __________ in the formulas.

• Ex: diphosphorus tetrafluoride = ________

Molecular Compounds Practice

• Write the name of the following compounds:

• Cl2O = __________

• NO =____________

• S2F10 = ____________

• P2S3 = _____________

More Molecular Compounds Practice

• Write the formula of the following:• Carbon tetrabromide =_________• Dinitrogen hexafluoride =________• Nitrogen Trichloride = _________• Phosphorus trihydride = _________

Homework/More Practice

• Write the following name for the compound or write the correct formula

• CI4 = _________• N2F6 = ________• Carbon trioxide = __________• Carbon monoxide =___________

Homework/More Practice

• P2O5 = ____________

• Nitrogen monoxide = __________

• CCl4 = ____________

• CBr3 = ___________

• Carbon tetraiodide = ___________

6-4 The Structure of Metals

• A________ bond is the attraction between a metal_______ and the shared ________ that surround it.

• The cation in a metal form a_______ that his held in place by the ________metallic bonds between the cations and the surrounding valence ___________

Metallic bonding• Although the electrons are moving

amoung the atoms, the _________number of electrons does not change

• The overall metal is __________• Metallic bonds in some metals

are________ than in other• _________metals are weaker compared to

__________ metals

Explaining Properties of Metals

• The _________ of electrons within a metal lattice explains some of the___________ of metals

• _________ and ability conduct an_________current are two properties

• An electric current can be carried through a metal by the flow of the shared _________

• ___________ – being able to be drawn into a thin wire is another property

Review Questions• What holds metal ions together in

a metal lattice?

• What characteristic of a metallic bond explains some of the properties of metals?

6-4 Continued Alloys• An _________ is a mixture of two or

more elements, at least one of which is a _______.

• Alloys have the characteristic__________ of metals

Copper Alloys• _________ was the first important alloy and is

associated with the bronze era.• Bronze contains only _______ and _______,

which are relatively soft metals• Mixed together in bronze, the metals are

much _________ and ___________ than either metal alone.

• Scientists can design alloys with specific properties by varying the________ and_______ of elements in an alloy

Steel Alloys• 1900’s was the Age of Steel because of

skyscrapers, automobiles, and ships were built from _________.

• Steel is an alloy of________ that contains small quantities of ______

• Stainless steels are durable because_________ forms an oxide that protects the steel from rusting

• _________ steel is more brittle than steels that contain more _______

Other Alloys• Airplane parts are made of many

different________• _______aluminum is lighter than

most metals, it ______ and______ too easily

• _______ and __________ is added to make the material stronger

Review Questions1. How can scientists design alloys

with specific properties?

2. Explain why the metallic bonds in some metals are stronger than the bonds in other metals