Entry Task: Nov. 13 th Friday Get papers in lab area Update Ch. 7 “I CAN” See what you are missing before test!

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.

ElementGroupPeriodFamily Metal nonmetal metalloid Standard E. Config Shorthand E.Config. # Ve- Astatine 25 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 2 [Kr] 5s 2 4d 10 5p halogen s non metal 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 5 [Xe]6s 2 4f 14 5d 10 6p 5 7 Strontium Akali Earth metals metals 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 [Kr]5s 2 2 Geranium 144 N/A metalloid [Ar]4s 2 3d 10 4p 2 4 Xenon 185 Noble Gas Non metal 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 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 H 2 O) 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 Fe 2 (SO 3 ) 3 ________________ (H 3 O) 3 BO 3 ________________ Hg 3 (PO 4 ) 2 ________________ Cu 2 CO 3 ________________ Al(NO 3 ) 3 ________________ Iron III sulfite Hydronium borate Mercury II phosphate Copper I carbonate Aluminum nitrate

For the following, provide the formula Gallium cyanide Ga +3 CN -1 Ga(CN) 3 Bismuth III chromate Bi +3 CrO 4 -2 Bi 2 (CrO 4 ) 3

Iron III hydroxide Fe +3 OH -1 Fe(OH) 3 Hydronium phosphide H 3 O +1 P -3 (H3O)3P(H3O)3P Copper I selenate Cu +1 SeO 4 -2 Cu 2 SeO 4

Flip paper over To Know List STUDY for P of U Ch. 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 Bring textbook to do Homework