4.1 ATOMIC

THEORY &

BONDING

4.1 VOCABULARYAlkali earth metalsAlkali metalsAnionsAtomic #Atomic numberAtomic TheoryAtoms Bohr diagramCations Chemical ChangeChemical reactionCompound Covalent bonding

MoleculeNeutronNoble gasesNon-MetalNucleusPeriodProtonPure SubstanceStable outer shellSubatomic particleTransition metalsValence electrons

Covalent CompoundElectronsElement Family/GroupHalogensIonic bondingIonic compoundsIonsLewis DiagramMatterMetalMetalloidsMixture

MechanicalSuspensions

Solutions Elements Compounds

No new substances produced

Only a change in state or appearance

New substances produced

Very hard to reverse

= CHEMICAL REACTION

• An atom is the smallest particle of an element that still has the properties of that element

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ATOMS

50 million atoms, lined up end to end = 1 cm

An atom = proton(s) + neutron(s) + electron(s)

Atoms join together to form compounds

A compound is a pure substance that is composed of two or more atoms combined in a specific way.

Oxygen and hydrogen are atoms/elements; H2O is a compound.

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COMPOUNDS

COMPOUNDS

A chemical change occurs when the arrangement of atoms in compounds changes to form new compounds.

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CHEMICAL CHANGE

Atoms are made up of smaller particles called subatomic particles.

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ATOMIC THEORY

• The nucleus is at the center of an atom

• The nucleus is composed of -positive protons and neutral neutrons

• Electrons exist in the space surrounding the nucleus.

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ATOMIC THEORY

# of protons = # of electrons in every atomNuclear charge = charge on the nucleus = # of protons

Nuclear charge = Atomic number Atomic number = # of protons = # of electrons

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ATOMIC THEORY

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ELEMENTSAtomic Number = smaller number

= number of p+ and e-

Atomic Mass = larger number= total of p+ and n0

28 +2 +3

Ni Nickel

58.71

Atomic Number

Atomic Mass

Combining Capacities

Symbol

Name of Element

CALCULATING NUMBER OF SUBATOMIC PARTICLES• Protons = same as atomic

number

• Electrons = same as atomic number

• Neutrons = subtract atomic number from atomic mass

PERIODIC TABLE PRACTICE

Element Symbol Atomic Number

Atomic Mass

Number of

Protons

Number of

Neutrons

Number of

Electrons

HydrogenBerylliumCarbon

Cobalt

Nickel

Krypton

THE PERIODIC TABLE

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Where are the following?• Atomic

number• Atomic Mass• Charges• Symbol• Name

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In the periodic table elements are listed in order by their atomic number.

Metals are on the leftThe transition metals range from group 3 -12Non-metals are on the rightMetalloids form a “staircase” toward the right side.

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Organization of the Periodic Table

Metals (left of zig zag line)Physical Properties of Metals: Shiny, good conductors of heat and electricity, ductile (make wires) and malleable (thin sheets). Easily lose electrons. Like to join with non-metals. Corrode (tarnish/rust).

Nonmetals (right of zig zag line)Physical Properties of Nonmetals: dull appearance, poor conductor, brittle (breaks easily), not ductile or malleable. Easily gain electrons. Like to join with metals, but will bond to other non-metals.

Metalloids (on both sides of zigzag line)Physical Properties of Metalloids: have properties of both metals and nonmetals. Solid, shiny or dull, ductile and malleable, conduct heat and electricity, but not very well.

THE PERIODIC TABLE

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Where are the following?• Metals• Non-metals• Transition

metals• Metalloids

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Rows of elements (across) are called periods.All elements in a period have their electrons in the same general area around their nucleus.

Example: period 3 all have 3 electron shells

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Organization of the Periodic Table

sodium magnesium aluminum

–Columns of elements are called groups, or families.• All elements in a family have similar properties and bond with other

elements in similar ways.• Group 1 = alkali metals• Group 2 = alkaline earth metals• Group 17 = the halogens• Group 18 = noble gases

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Organization of the Periodic Table

17

18

Group 1 = alkali metalsvery reactive metalswant to give away 1 electronie: lithium, sodium, potassium...

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Organization of the Periodic Table

1 2 17

18

Group 2 = alkali earth metalssomewhat reactive metalswant to give away 2 electronsie: beryllium, magnesium, calcium...

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Organization of the Periodic Table

1 2 17

18

Group 17 = halogensvery reactive non-metalswant to accept 1 electronreact with alkali metalsie: fluorine, chlorine, bromine......

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Organization of the Periodic Table

1 2 17

18

Group 18 = noble gasesSTABLE. Very non reactive gaseous non-metalsie: helium, neon, argon......

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Organization of the Periodic Table

1 2 17

18

THE PERIODIC TABLE

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Where are the following?• Period• Group/Family• Alkali metals• Alkaline earth

metals• Halogens• Noble gases

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Atoms gain and lose electrons to form bonds.The atoms become electrically charged particles called

ions.

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Periodic Table & Ion Formation

Atoms gain and lose electrons to form bonds.Metals lose negative electrons & become positive ions.

Positive ions are called CATIONS.

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Periodic Table & Ion Formation

Some metals are MULTIVALENT and can lose a varying number of electrons.

For example, iron, Fe, loses either two (Fe2+) or three (Fe3+) electrons

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Periodic Table & Ion Formation

Atoms gain and lose electrons to form bonds.Non-metals gain electrons and become negative ions

Negative ions are called ANIONS

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Periodic Table & Ion Formation

Atoms gain and lose electrons in an attempt to be STABLE.The noble gases are stable because they have FULL outer

shells of electrons. They don’t need to lose or gain any e-s.Atoms in each period want to have the same number of

electrons in their outer shell (VALENCE ELECTRONS) as the noble gases on the end of their period.

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Periodic Table & Ion Formation

Bohr diagrams show how many electrons appear in each electron shell around an atom.

The first electron shell holds 2 electronsThe second electron shell holds 8 electronsThe third electron shell holds 8 electronsThe fourth electron shell holds 18 electrons

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BOHR MODELS

The noble gas elements have full electron shells and are very stable = STABLE OCTET

Electrons appear in shells in a very predictable manner.

The period number = the number of shells in the atom.Except for the transition elements (family 3-12), the last

digit of the group number = the number of electrons in the valence shell.

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Patterns of Electron Arrangement in Periods &

Groups

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•It has 2 + 8 + 8 = 18 electrons, and therefore, 18 protons.

•It has three electron shells, so it is in period 3.

•It has eight electrons in the outer (valence) shell.

BOHR MODELSWhat is the Bohr Model Diagram for Argon?