Section 2.1 The Structure of the Atom. The Structure of the Atom In this section… a.The components of an atom b.Atomic symbols c.Isotopes and atomic weight.

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Presentation transcript:

Section 2.1 The Structure of the Atom

The Structure of the Atom In this section… a.The components of an atom b.Atomic symbols c.Isotopes and atomic weight

The Structure of the Atom Components of an Atom:

The Structure of the Atom Components of an Atom:

The Structure of the Atom

Atomic number and mass number:

The Structure of the Atom Atomic symbols:

The Structure of the Atom Isotopes: atoms with the same number of protons but different numbers of neutrons

The Structure of the Atom Isotopes and average atomic weight: The average atomic weight of an element depends on the mass of the atoms but also on the relative abundance of each isotope.

The Structure of the Atom Average atomic weights are shown on periodic table:

Chiuaua: 4 lbs. Mastif: 120 lbs. What is the average weight of a collection of these dogs?

The Structure of the Atom Isotopes and average atomic weight: Average dog mass: 96 % 4 lbs. 4 % 120 lbs.

The Structure of the Atom Elements with a single isotope have atomic weight = mass of that isotope Can make rough estimate of relative abundance from average atomic weight.

Isotope trends among the elements:

The Structure of the Atom Isotopes and average atomic weight: how do we know all this? Mass spectrometry

Section 2.2 Elements and the Periodic Table

The Periodic Table In this section… a.Structure of the periodic table b.Classifications of elements c.Element structures (atomic arrangements)

Periodic table structure: groups (columns)

Periodic table structure: periods (rows)

Periodic table structure: main group elements

Periodic table structure: transition metals

Periodic table structure: lanthanides and actinides

Classification of elements:

Periodic trends: density

Periodic trends: melting point

Element structures

Element structures: extended structures

Element structures: allotropes (same element, different structures)

Section 2.3 Covalent Compounds

Covalent Compounds In this section… a.The nature of covalent compounds b.Ways of representing covalent compounds c.Naming covalent compounds

Covalent Compounds Covalent compounds are composed of atoms of different elements that are bonded together by sharing electrons. Two types: -- molecular compounds -- network covalent compounds

Covalent Compounds Molecular compounds: composed of individual molecules containing the same number of atoms

Covalent Compounds Molecular compounds: composed of individual molecules containing the same number of atoms

Molecular Compounds Molecular compounds: carbondioxide

Covalent Compounds Network covalent compounds: A large number of atoms of different elements bonded by shared electrons. Each sample has molecules with different numbers of atoms.

Covalent Compounds Network covalent compounds: silicondioxide

Covalent Compounds Representing compounds: Molecular formula: depicts number of atoms of each element Empirical formula: shows simplest integer ratio of atoms of each element Structural formula: shows atomic linkages Models: show 3-dimensional shape of molecule

Covalent Compounds Molecular formula: depicts number of atoms of each element

Covalent Compounds Empirical formula: shows simplest integer ratio of atoms of each element molecular formula: empirical formula:

Covalent Compounds Molecular and Empirical formulas are often the same.

Covalent Compounds Structural formula: shows connections between atoms

Covalent Compounds Condensed structural formula: mainly for organics. CH 3 CH 2 CH 2 CH 2 OH

Covalent Compounds Models: show 3-dimensional shape wedge-and-dash ball-and-stick

Covalent Compounds Models: Ball-and-Stick vs. Space Filling

Nomenclature: Naming Binary Nonmetal Compounds Going from formula to name. Interactive Table 2.3.1

1. The first word in the compound name is the name of the first element in the compound formula. If the compound contains more than one atom of the first element, use a prefix (Table 2.3.2) to indicate the number of atoms in the formula. CS 2 First word in compound name: carbon N 2 O 4 First word in compound name: dinitrogen 2. The second word in the compound name is the name of the second element in the formula that has been changed to end with -ide. In all cases, use a prefix (Table 2.3.2) to indicate the number of atoms in the formula. CS 2 Second word in compound name: disulfide N 2 O 4 Second word in compound name: tetraoxide 3. The compound is named by combining the first and second words of the compound name. CS 2 carbon disulfide N 2 O 4 dinitrogen tetraoxide

Some Examples: SO 2 SO 3 ClO S 2 F 10 Some Common Compounds: H 2 O N 2 H 4 H 2 O 2 NO NH 3

Important Simple Hydrocarbons Alkanes: Table Hydrocarbon Name CH 4 Methane C 2 H 6 Ethane C 3 H 8 Propane C 4 H 10 Butane C 5 H 12 Pentane C 6 H 14 Hexane C 7 H 16 Heptane C 8 H 18 Octane C 9 H 20 Nonane C 10 H 22 Decane

Table 2.3.5: Names and Formulas of the Halogen Oxoacids Name Formula HClO 4 Perchloric acid HBrO 4 Perbromic acid HIO 4 Periodic acid HClO 3 Chloric acid HBrO 3 Bromic acid HIO 3 Iodic acid HClO 2 Chlorous acid HBrO 2 Bromous acid HIO 2 Iodous acid HClO Hypochlorous acid HBrO Hypobromous acid HIO Hypoiodous acid

Table 2.3.6: Names and Formulas of Some Inorganic Acids Name Formula Hydrogen chloride HCl (also hydrochloric acid) Hydrogen bromide HBr (also hydrobromic acid) Hydrogen iodideHI(also hydroiodic acid) Nitric acid HNO 3 Nitrous acid HNO 2 Hydrogen sulfide H 2 S Sulfuric acid H 2 SO 4 Sulfurous acid H 2 SO 3 Phosphoric acid H 3 PO 4

Section 2.4 Ionic Compounds

Ionic Compounds In this section… a.Monatomic and Polyatomic ions b.Ionic compound formulas c.Naming ionic compounds d.Covalent vs. Ionic compounds

Formation of Ions Cations: Positive ions form by loss of electrons.

Formation of Ions Anions: Negative ions form by gain of electrons.

Names of Monatomic Ions monatomic cations: element name + “ion” monatomic anions: element name with “ide” suffix + “ion”

Common Monatomic Ions

Naming Transition Metal Cations The name of a transition metal cation is the element name followed by the cation charge in Roman numerals within parentheses and the word ion. Cr 2+ Co 3+

Polyatomic Ions Groups of bonded atoms with a charge Ammonium ion: NH 4 + Carbonate ion: CO 3 2-

Table 2.4.1: Polyatomic Ions

Formulas of Ionic Compounds Rule: Total charge on cations = Total charge on anions So, ions combine in numbers so charges cancel. Mg 2+ and Cl - Mg 2+ and N 3- Mg 2+ and O 2- Na + and O 2-

Formulas of Ionic Compounds Rule: Total charge on cations = Total charge on anions When multiple polyatomic ions are present, they are in parentheses. Mg 2+ and PO 4 3- Parentheses are not used with a single polyatomic ion: Mg 2+ and SO 4 2-

Formulas of Ionic Compounds Ionic compounds are extended structures: No molecules, so no “molecular formula.”

Naming Ionic Compounds Ionic compound name = cation name + anion name The word “ion” is dropped from the ion names. The name does NOT reflect the number of ions. NaCl MgCl 2 Na 2 SO 4 (NH 4 ) 3 PO 4

Naming Ionic Compounds Transition metals with variable charges? The name of a transition metal cation is the element name followed by the cation charge in Roman numerals within parentheses and the word ion. CrCl 2 CoPO 4

Identifying Covalent vs. Ionic Compounds Metals + nonmetals Metals + polyatomic anions Two polyatomic ions Two nonmetals, but no polyatomic ions Ionic Compounds: Covalent Compounds: