Chemistry Chapter 2. Atoms, Molecules, and Ions Section Periodic Table Ions Chemical Bonds Nomenclature

Transcription

1 Chemistry Chapter 2 Atoms, Molecules, and Ions Section Periodic Table Ions Chemical Bonds Nomenclature

2 Organization of the Periodic Table Columns, Groups or Families elements in the same vertical columns ranges from 1 to 18 Periods horizontal rows of elements ranges from 1 to 7

3 Organization of the Periodic Table Periodic Table can be divided by Metallic Character Metals Nonmetals Metalloids

4 Organization of the Periodic Table Periodic Table can be arranged by blocks s Block p Block d Block f Block Blocks

5 Organization of the Periodic Table Periodic Table can be arranged by Family Names Alkali Metals Alkaline Earth Metals Halogens Noble Gases Transition Metals Lanthanides Actinides Family Names

6 Organization of the Periodic Table Periodic Table can be arranged by Other Blocks Main Group Elements Transition Metals Inner Transition Metals Other Blocks

7 Ionization Any process that results in the formation of an ion Ion atom, or group of atoms, that has a net positive or negative charge Cation positive ion [loses electron(s)] Anion negative ion [gains electron(s)] Remember, an electron has a negative charge so if you lose an electron [ -(1-)] it is positive (cation) if you gain an electron [+(1-)] it is a negative (anion)

8 Ionization Ions are shown using the symbol with a superscript after the symbol showing the charge Remember that the number comes before the charge but we say the charge then the number H H 1+ O O 2- Hydrogen Atom Hydrogen Ion (or Hydrogen Cation) Oxygen Atom Oxygen Ion (or Oxygen Anion)

9 Ionization Table of common charges formed when creating ionic compounds of the Main Group elements Group Name Charge 18 Noble Gases 0 1 Alkali Metals 1+ 2 Alkaline Earth Metals Group Halogens 1-16 Group Group 15 3-

10 Concept Check What ion does each atom want to form? Li F O Li 1+ Ca Ca 2+ F 1- Al Al 3+ O 2- N N 3-

11 Types of Chemical Bonds Two types of Chemical Bonds: Ionic Bonds Covalent Bonds

12 Types of Chemical Bonds Ionic Bonds Bonds form due to force of attraction between oppositely charged ions Resulting collection of atoms is called a Formula Unit Shows the simplest whole number ratio between the atoms Always an empirical formula (simplest ratio)

13 Types of Chemical Bonds Covalent Bonds Bonds form between atoms by sharing electrons Resulting collection of atoms is called a Molecule Shows the exact combination of atoms that form a molecule

14 Binary Compounds Composed of two elements Includes both: Binary Ionic Compound Metal and a Nonmetal Binary Covalent Compound Nonmetal and Nonmetal When naming compounds, get out the guns

15 Binary Ionic Compounds The cation is always first and the anion second A monatomic cation takes its name from the name of the parent element A monatomic anion is named by taking the root of the element name and changing the end to ide Use the cross over to get the correct formula Make sure to clean it up : ones, simplify, parentheses

16 Binary Ionic Compounds Examples: KCl MgBr 2 CaO Potassium Chloride Magnesium Bromide Calcium Oxide Sodium Bromide Boron Nitride Potassium Oxide NaBr BN K 2 O

17 Binary Ionic Compounds Extended transition metals tend to form more than one type of cation The charge on the metal ion must be specified Roman numeral indicates the charge of the metal cation [Iron(II) for Fe 2+ ] Use the reverse cross-over to determine the charge Move numbers up to charges Check anion first; adjust if necessary Charge is what is on the cation

18 Binary Ionic Compounds Examples: CuBr FeS PbO 2 Copper (I) Bromide Iron (II) Sulfide Lead (IV) Oxide Copper (II) Chloride Iron (III) Nitride Mercury (I) Sulfide CuCl 2 FeN Hg 2 S

19 Polyatomic Ions Ions that contain a group of atoms The group cannot be separated; treat it as just one thing; use parenthesis if needed

20 Polyatomic Ions

21 Polyatomic Ions Examples: NaOH Cu(NO 3 ) 2 (NH 4 ) 2 SO 4 Sodium Hydroxide Copper (II) Nitrate Ammonium Sulfate Lead (IV) Carbonate Iron (II) Nitrate Ammonium Phosphate Pb(CO 3 ) 2 Fe(NO 3 ) 2 (NH 4 ) 3 PO 4

22 Binary Covalent Compounds Formed between two nonmetals Uses prefixes to indicate number of atoms

23 Binary Covalent Compounds 1. The first element in the formula is named first, using the full element name 2. The second element is named as if it were an anion (ending changed to ide) 3. Prefixes are used to denote the numbers of atoms present 4. The prefix mono- is never used for naming the first element

24 Binary Covalent Compounds Examples: CO 2 SF 6 N 2 O 4 Carbon Monocarbon Dioxide Dioxide Sulfur Hexafluoride Dinitrogen Tetroxide Carbon Monoxide Sulfur Trichloride Triphosphorous Pentabromide CO SCl 3 P 3 Br 5

25 Concept Check Which of the following compounds is named incorrectly? a) KNO 3 potassium nitrate b) Ag 2 O silver (I) oxide c) Sn(OH) 4 tin(iv) hydroxide d) PBr 5 phosphorus pentabromide e) CaCrO 4 calcium chromate

26 Naming Acids Acids can be recognized by the hydrogen that appears first in the formula HCl Molecule with one or more H + ions attached to an anion (monatomic or polyatomic) Add number of Hydrogens needed to balance anion

27 Naming Acids If the anion does not contain oxygen, the acid is named with the prefix hydro followed by the base unit with the suffix ic Examples: HCl HCN H 2 S Hydrochloric Acid Hydrocyanic Acid Hydrosulfuric Acid

28 Naming Acids If the anion does contain oxygen: The suffix ic is added to the root name if the anion name ends in ate Examples: HNO 3 H 2 SO 4 HC 2 H 3 O 2 Nitrate Sulfate Acetate Nitric Acid Sulfuric Acid Acetic Acid

29 Naming Acids If the anion does contain oxygen: The suffix ous is added to the root name if the anion name ends in ite Examples: HNO 2 H 2 SO 3 HClO 2 Nitrite Sulfite Chlorite Nitrous Acid Sulfurous Acid Chlorous Acid

30 Nomenclature Hints Get out the guns and find the elements For ionic compounds, formulas must balance out the charges For molecules, just tell what is there Do not use 1 s Do not use parenthesis if there is only one Always simplify ionic compound (not molecules) Be careful of the -ides, -ites, & -ates Be aware of acids

31 Chemistry Chapter 2 Section 2 Homework Set pg 66: #32, 33, 35, 56, 57, 59, 63, 67, 68, 70, 71, 75, 76, 79, 80, 81, 82, 97, 100, 113 (20)