Post on 18-Jan-2016
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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
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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