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Update Ch. 7 “I CAN”

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Agenda

• Sign off on Ch. 2-7 Review• Update Ch. 7 I Can• Look at Ionic Substances POGIL• Quiz on Ionic substances LT#4• Discuss 2-7 Review ws• IONIC BATTLESHIP!!!!• Y.T. TURN IN ALL LATE ASSIGNMENTS

Ch. 2-7 Review

EXPLAIN the difference between a physical property and chemical property. Provide an example of each.

• A physical property is the substances physical state- water is a liquid and transparent.

• A chemical property is the ABILITY of how a substance WILL behave in the presence of another substance- water is not flammable.

Place the following from smallest to largest: compound, atoms, elements and

mixture.• Smallest: Atom which make up

elements. • Elements bond to make

compounds. Compounds/substances can be mixed with other substances to make mixtures.

Describe what happens to a sodium atom if we remove: a proton, a neutron and an

electron.• Sodium has 11 protons, if it lost

a proton it would be neon.• Sodium has 12 neutrons, if it

lost a neutron it would be an isotope of sodium.

• Sodium has 11 electrons, if it lost a electron it would be a cation having a +1 charge.

Element Group Period FamilyMetal

nonmetalmetalloid

Standard E. Config ShorthandE.Config. # Ve-

Astatine

2 5

1s22s22p63s23p6

4s23d104p2

[Kr] 5s24d105p6

17 6 halogens

nonmetal

1s22s22p63s23p64s23d10

4p65s24d105p66s24f14

5d106p5

[Xe]6s24f14

5d106p5 7

StrontiumAkaliEarth metals

metals1s22s22p63s23p64s23d10

4p65s2 [Kr]5s2 2

Geranium 14 4 N/A metalloid [Ar]4s23d104p2 4

Xenon 18 5 Noble Gas

Nonmetal

1s22s22p63s23p64s23d10

4p65s24d105p6 8

What happens to the atom size as one moves through a group? Period?

In a group, the number of orbitals increases, thus increasing the atom’s size as you move down.

In a period, the nuclear charge increases as you move across so pulls the valence electrons closer so they atom sizes gets smaller.

What happens to the ionization energy as on moves through a group? Period?

In a group, the number of orbitals increases so the energy needed to remove a valence electron is low.

In a period, the number of valence electrons increases so the energy needed to remove a ve- is high.

What does electronegativity have to do with ionic bonding?

Electronegativity is the “want” for electrons.

Nonmetals have a high electronegativity, thus gains electrons (from metals) to have a fill orbit.

This transfer of electron(s) occurs during ionic bonding.

What is a chemical bond?

• A force that holds 2 or more atoms together.

Why do ions form?

• They lose or gain electrons to have a stable electron arrangement.

What family of elements is relatively unreactive and why?

• Noble Gases are unreactive because they have a filled valence orbit.

Describe the formation of cation and how does this relate to ionization

energy?

• Atoms lose their valence electrons becoming a positive charge because metals (cations) have low ionization energy.

Describe the formation of anion and how does this relate to electronegativity?

• Atoms gain electrons becoming a negative charge because they have high electronegativity “wanting” electrons.

Explain the formation of the ionic compound composed of lithium and

oxygen.

• 2 Lithium atoms loses their valence electron becoming +1 charge.

• Oxygen gains both of those electrons becoming a -2 charge.

• They fill create a stable orbital arrangement

• Cancel each other charges out.

Provide the 5 properties of an Ionic substance.

• High melting point• Dissolves in water• Conductive (after being dissolved in H2O)• Solids at room temperature• Brittle (not malleable)

What is the difference between a formula unit, and crystal lattice?

• Formula Unit is the simplest form of an ionic compound- NaCl.

• Crystal Lattice is the repeating formula unit forming a lattice.

NaClNaClNaClNaCl

NaClNaClNaCl

NaClNaClNaClNaCl

NaClNaClNaCl

What is the difference between a monatomic ion and a polyatomic ion?

• Monatomic ion is a one atom ion.• Polyatomic ion is a 2 or more atoms that

are covalently bonded that carry a charge.

For the following, provide the correct names

Fe2(SO3)3________________(H3O)3BO3________________Hg3(PO4)2________________Cu2CO3________________Al(NO3)3________________

Iron III sulfite

Hydronium borateMercury II phosphateCopper I carbonate

Aluminum nitrate

For the following, provide the formula

Gallium cyanide

Ga+3 CN-1

Ga(CN)3

Bismuth III chromate Bi+3 CrO4

-2

Bi2(CrO4)3

Iron III hydroxide Fe+3 OH-1

Fe(OH)3

Hydronium phosphide H3O+1 P-3

(H3O)3P

Copper I selenate Cu+1 SeO4

-2

Cu2SeO4

Flip paper overTo Know List

STUDY for P of UCh. 3-8

To Know

Ch. 8 Test

• Concentration of MOSTLY Ch. 8 (55%)– Why bond?– Ionic substances- properties– Naming ionic substances– Providing the formula– Transitional metals- ROMAN

NUMERALS– Binary compounds vs. polyatomic

compounds

To Know

Ch. 8 Test

• Concentration of MOSTLY Ch. 8 (55%)– Periodic trends-

• Ionization energy• Electronegativity• Size of atoms verse ions

– Energy levels-light, E-dot/valence-Ch. 5– Particles- Protons, Electrons Neutrons-Ch.

4– Physical chemical properties/changes-Ch.

3

45%

STUDY for P of U Ch. 3-8

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