Atoms, Ions, Molecules

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  • Identify types of substances: Atom, Ion, Molecule

    • Substances shown:

      • H

      • Mg

      • Mg

      • H

      • H

      • H

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  • Definition of Atom

    • Tiny indivisible particle of an element

    • Each element has one kind of atom

    • 118 known chemical elements

    • Atoms are neutral

    • Examples:

      • Oxygen (O)

      • Hydrogen (H)

      • Sodium (Na)

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  • Atomic Structure

    • Composed of:

      • Neutrons

      • Electrons

      • Nucleus (contains Protons)

    • Electrons are found in electron clouds or orbitals

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  • Carbon Atom Structure

    • Protons (p+) = 6

    • Electrons (e) = 6

    • Neutrons (n°) = 6

    • Atomic Mass: 12.0107

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  • Oxygen Atom Structure

    • Protons (p+) = 8

    • Electrons (e) = 8

    • Neutrons (n°) = 8

    • Atomic Mass: 15.9994

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  • Atom Notation

    • Notation format: XA

      • Z: Atomic Number = number of protons

      • Mass Number = number of protons + neutrons

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  • Hydrogen Atom Notation

    • Notation: H1

    • Atomic Number = 1

    • Mass Number = 1

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  • Example of Elements with Protons, Electrons & Neutrons

    • Element:

      • Element: 11 Proton: 11 Neutron: 12

      • Element: 17 Proton: 17 Neutron: 18

      • Element: 7 Proton: 7 Neutron: 7

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  • Summary Table

    • Symbol | Atomic # | Atomic Mass | Proton | Electron | Neutron

      • C | 6 | 12 | 6 | 6 | 6

      • K | 19 | 39 | 19 | 19 | 20

      • Cu | 29 | 64 | 29 | 29 | 35

      • Sn | 50 | 119 | 50 | 50 | 69

      • Au | 79 | 197 | 79 | 79 | 118

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  • Isotopes

    • Definition: Atoms with the same atomic number but different mass numbers

    • Examples:

      • Protium (1H)

      • Deuterium (2H)

      • Tritium (3H)

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  • Uses of Isotopes

    • Uranium-235

      • Used as fuel for nuclear reactors

    • Uranium-238

      • Determining age of marine sediments

    • Carbon-14

      • Carbon dating for archaeological materials

    • Iodine-131

      • Treatment for thyroid cancer

    • Technetium-99

      • Imaging for diagnostics

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  • Additional Uses of Isotopes

    • Cobalt-60

      • Radiation for cancer treatment

    • Thallium-201

      • Assessment for heart tissue damage

    • Americium-241

      • Thickness measurement in steel and paper

    • Californium-252

      • Moisture content measurement in construction

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  • Atoms combine to form Molecules or Ions

    • Electrons may be lost or gained

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  • Ion Formation

    • Loss of electrons: Cation

    • Gain of electrons: Anion

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  • Definition of Ion

    • Formed when an atom loses or gains electrons

    • Types:

      • Monoatomic (e.g., N3-, Ba2+)

      • Polyatomic (e.g., CO3 2-)

    • Positive ions (cations) or negative ions (anions)

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  • Classification of Elements: Metals, Nonmetals, and Metalloids

    • Examples of Metals:

      • Na, Mg, Al

    • Examples of Nonmetals:

      • C, O, N

    • Metalloids: Boron (B), Silicon (Si), etc.

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  • Naming Monoatomic Ions

    • Examples:

      • Group 1A: Na+ (Sodium ion)

      • Group 2A: Mg2+ (Magnesium ion)

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  • Transition Metals

    • Vary in number of electrons lost

    • Naming Methods: Classical & Stock

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  • Classical Naming Method

    • Suffixes:

      • -ous = lower charge (e.g., Fe2+ = Ferrous)

      • -ic = higher charge (e.g., Fe3+ = Ferric)

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  • Examples of Classical vs. Stock Method

    • Cu+ = Cuprous ion

    • Cu2+ = Cupric ion

    • Sn2+ = Stannous ion

    • Sn4+ = Stannic ion

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  • Stock Naming Method

    • Roman numeral indicates charge in parentheses

    • Example: Fe2+ = Ferrous iron (II)

    • Example: Fe3+ = Ferric iron (III)

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  • Examples of Naming Ions in Stock Method

    • Cu+ = Copper (I)

    • Cu2+ = Copper (II)

    • Sn2+ = Tin (II)

    • Sn4+ = Tin (IV)

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  • Naming Monoatomic Anions

    • Examples:

      • S2- = Sulfide ion

      • Br- = Bromide ion

      • F- = Fluoride ion

      • O2- = Oxide ion

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  • Naming Polyatomic Anions

    • Examples:

      • OH- = Hydroxide ion

      • CN- = Cyanide ion

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  • Naming Polyatomic Anions with Oxygen

    • Examples:

      • NO2- = Nitrite ion

      • NO3- = Nitrate ion

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  • Naming Anions with Sulfur Substitution

    • Examples:

      • OCN- = Cyanate ion

      • SCN- = Thiocyanate ion

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  • Definition of Molecule

    • Formed by nonmetals sharing electrons

      • Diatomic or Polyatomic

      • Examples:

        • H2O, H2S, C6H12O6, C10H8

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  • Diatomic Molecules

    • Nonmetallic elements that exist as diatomic molecules

      • Examples:

        • N2, O2, H2, F2, Cl2

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  • Molecular Compounds

    • Composed of different elements, can be diatomic or polyatomic

      • Examples:

        • HCl, HBr, H2S, H2O, CO2

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  • Naming Molecular Compounds

    • Use Greek prefixes for both elements

    • Add suffix -ide to the second element

    • Example: SF6 = Sulfur hexafluoride

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  • Greek Prefixes for Naming:

    • 1 = mono-

    • 2 = di-

    • 3 = tri-

    • 4 = tetra-

    • 5 = penta-

    • 6 = hexa-

    • 7 = hepta-

    • 8 = octa-

    • 9 = nona-

    • 10 = deca-

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  • Naming Examples

    • P2S3 = Diphosphorus trisulfide

    • CF3 = Carbon trifluoride

    • P2O5 = Diphosphorus pentaoxide

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  • Summary on Ion Naming

    • Monoatomic Ion (Cation):

      • Unchanged name for groups 1A and 2A

      • Transition metals: Classical or Stock naming

    • Monoatomic Ion (Anion):

      • Root name + suffix -ide

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  • Summary on Polyatomic and Molecular Compounds

    • Polyatomic Ion: Atomic constituent + suffix –ide

    • Polyatomic Ion with Oxygen:

      • Root name + -ite (lesser)

      • Root name + -ate (greater)

    • Molecular Compounds: Greek prefixes + -ide suffix