Chemistry 1 Chapter 7 PO 43 phosphate ion

Chemistry 1: Chapter 7 PO 43 phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 acetate ion SAVE PAPER AND INK!!! When you print out the notes on Power. Point, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

Forms of Chemical Bonds Most bonds are somewhere in between ionic and covalent. • There are 3 forms bonding atoms: • Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) • Covalent—some valence electrons shared between atoms • _____ – holds atoms of a metal together

Common Names • A lot of chemicals have common names as well as the proper IUPAC name. • Chemicals that should always be named by common name and never named by the IUPAC method are: • H 2 O water, not dihydrogen monoxide • NH 3 ammonia, not nitrogen trihydride

COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl- --> Na. Cl A neutral compound requires equal number of + and - charges.

Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 Cd+2 0

Properties of Ionic Compounds Forming Na. Cl from Na and Cl 2 • A metal atom can transfer an electron to a nonmetal. • The resulting cation and anion are attracted to each other by electrostatic forces.

IONIC COMPOUNDS NH 4 + Cl ammonium chloride, NH 4 Cl

Some Ionic Compounds Ca 2+ + 2 F- ---> Ca. F 2 Mg 2+ + N-3 ----> Mg 3 N 2 magnesium nitride Sn 4+ + O 2 - ----> Sn. O 2 Tin (IV) oxide calcium fluoride

Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions Na + F : sodium + fluorine Charge balance: Na+ – : F : Na. F sodium fluoride 1+ 1 - formula = 0

Monatomic Ions

Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl. Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl Cl 3. Write the number of ions needed as subscripts Ba. Cl 2

Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+, S 2 a) Na. S b) Na 2 S c) Na. S 2 2. Al 3+, Cla) Al. Cl 3 b) Al. Cl c) Al 3 Cl 3. Mg 2+, N 3 a) Mg. N b) Mg 2 N 3 c) Mg 3 N 2

Solution 1. Na+, S 2 b) Na 2 S 2. Al 3+, Cla) Al. Cl 3 3. Mg 2+, N 3 c) Mg 3 N 2

Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca 2+ = calcium ion • 3. Monatomic anion = root + -ide • Cl = chloride • Ca. Cl 2 = calcium chloride

Naming Binary Ionic Compounds l Examples: Na. Cl sodium chloride Zn. I 2 zinc iodide Al 2 O 3 aluminum oxide

Learning Check Complete the names of the following binary compounds: Na 3 N sodium ________ KBr potassium ________ Al 2 O 3 aluminum ________ Mg. S _____________

Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ Cu+, Cu 2+ copper(I) ion copper (II) ion 2+ or 3+ Fe 2+, Fe 3+ iron(II) ion iron(III) ion

Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1 A, 2 A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4 A and 5 A (except Ag, Zn, Cd, and Al) require a Roman Numeral. Fe. Cl 3 Cu. Cl Sn. F 4 Pb. Cl 2 Fe 2 S 3 (Fe 3+) (Cu+ ) (Sn 4+) (Pb 2+) (Fe 3+) iron (III) chloride copper (I) chloride tin (IV) fluoride lead (II) chloride iron (III) sulfide

Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

Learning Check Complete the names of the following binary compounds with variable metal ions: Fe. Br 2 iron (_____) bromide Cu. Cl copper (_____) chloride Sn. O 2 ___(_____ ) _______ Fe 2 O 3 ____________ Hg 2 S ____________

Polyatomic Ions NO 3 nitrate ion NO 2 nitrite ion

Polyatomic Ions You can make additional polyatomic ions by adding a H+ to the ion! CO 3 -2 is carbonate HCO 3– is hydrogen carbonate H 2 PO 4– is dihydrogen phosphate HSO 4– is hydrogen sulfate

Ternary Ionic Nomenclature Writing Formulas • Write each ion, cation first. Don’t show charges in the final formula. • Overall charge must equal zero. • If charges cancel, just write symbols. • If not, use subscripts to balance charges. • Use parentheses to show more than one of a particular polyatomic ion. • Use Roman numerals indicate the ion’s charge when needed (stock system)

Ternary Ionic Nomenclature Sodium Sulfate Na+ and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe+3 and OHFe(OH)3 Ammonium carbonate NH 4+ and CO 3 – 2 (NH 4)2 CO 3

Learning Check 1. aluminum nitrate a) Al. NO 3 b) Al(NO)3 c) Al(NO 3)3 2. copper(II) nitrate a) Cu. NO 3 b) Cu(NO 3)2 c) Cu 2(NO 3) 3. Iron (III) hydroxide a) Fe. OH b) Fe 3 OH 4. Tin(IV) hydroxide a) Sn(OH)4 b) Sn(OH)2 c) Fe(OH)3 c) Sn 4(OH)

Naming Ternary Compounds l Contains at least 3 elements l There MUST be at least one polyatomic ion (it helps to circle the ions) l Examples: Na. NO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3)3 Aluminum bicarbonate or Aluminum hydrogen carbonate

Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite Mg. SO 3 b) magnesium sulfate Mg. SO 4 c) sodium carbonate 2. Ca(HCO 3)2 a) calcium carbonate Ca. CO 3 Ca 3(PO 4)2 b) calcium phosphate c) calcium bicarbonate

Mixed Practice! Name the following: 1. Na 2 O 2. Ca. CO 3 3. Pb. S 2 4. Sn 3 N 2 5. Cu 3 PO 4 6. Hg. F 2

Mixed Up… The Other Way Write the formula: 1. Copper (II) chlorate 2. Calcium nitride 3. Aluminum carbonate 4. Potassium bromide 5. Barium fluoride 6. Cesium hydroxide

Naming Molecular Compounds CO 2 Carbon dioxide CH 4 methane BCl 3 boron trichloride All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (Na. Cl)

Molecular (Covalent) Nomenclature for two nonmetals • Prefix System (binary compounds) 1. Less electronegative atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3. Change the ending of the second element to -ide.

Molecular Nomenclature Prefixes PREFIX monoditritetrapentahexaheptaoctanonadeca- NUMBER 1 2 3 4 5 6 7 8 9 10

Molecular Nomenclature: Examples • CCl 4 • carbon tetrachloride • N 2 O • dinitrogen monoxide • SF 6 • sulfur hexafluoride

More Molecular Examples • arsenic trichloride • As. Cl 3 • dinitrogen pentoxide • N 2 O 5 • tetraphosphorus decoxide • P 4 O 10

Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon ________ PCl 3 phosphorus _______chloride CCl 4 carbon ____chloride N 2 O _____nitrogen _____oxide

Learning Check 1. P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

A flow chart for naming compounds.

Mixed Review Name the following compounds: 1. Ca. O a) calcium oxide c) calcium (II) oxide 2. 3. Sn. Cl 4 a) tin tetrachloride c) tin(IV) chloride N 2 O 3 a) nitrogen oxide c) nitrogen trioxide b) calcium(I) oxide b) tin(II) chloride b) dinitrogen trioxide

Solution Name the following compounds: 1. Ca. O a) calcium oxide 2. Sn. Cl 4 c) tin(IV) chloride 3. N 2 O 3 b) Dinitrogen trioxide

Mixed Practice 1. 2. 3. 4. 5. 6. 7. 8. 9. Dinitrogen monoxide Potassium sulfide Copper (II) nitrate Dichlorine heptoxide Chromium (III) sulfate Iron (III) sulfite Calcium oxide Barium carbonate Iodine monochloride

Mixed Practice 1. 2. 3. 4. 5. 6. 7. 8. 9. Ba. I 2 P 4 S 3 Ca(OH)2 Fe. CO 3 Na 2 Cr 2 O 7 I 2 O 5 Cu(Cl. O 4)2 CS 2 B 2 Cl 4

Acid Nomenclature • Acids • Compounds that form H+ in water. • Formulas usually begin with ‘H’. • In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) • Ternary acids are ALL aqueous • Examples: • HCl (aq) – hydrochloric acid • HNO 3 – nitric acid • H 2 SO 4 – sulfuric acid

Acid Nomenclature Review No Oxygen w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

Acid Nomenclature Flowchart

Acid Nomenclature • HBr (aq) • No oxygen, -ide hydrobromic acid carbonic acid sulfurous acid • H 2 CO 3 • Has oxygen, -ate • H 2 SO 3 • Has oxygen, -ite

Acid Nomenclature • hydrofluoric acid • 2 elements H+ F- HF (aq) • sulfuric acid • 3 elements, -ic H+ SO 42 - H 2 SO 4 • nitrous acid • 3 elements, -ous H+ NO 2 - HNO 2

Name ‘Em! • HI (aq) • HCl • H 2 SO 3 • HNO 3 • HIO 4

Write the Formula! • Hydrobromic acid • Nitrous acid • Carbonic acid • Phosphoric acid • Hydrotelluric acid

Now it’s Study Time DONE

Rainbow Matrix Game • Link on Chemistry Geek. com on Chemistry I page • http: //chemistrygeek. com/rainbow Use [ ] to represent subscripts since you can’t enter subscripts into the computer So H 2 O would be H[2]O And Al 2(SO 4)3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3 -3 ; Silicate = Si. O 4 -4 ; Manganate = Mn. O 4 -2 (permanganate is -1)