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Chemical Names and Formulas

Explore the world of chemical names and formulas, from molecular compounds to ionic compounds. Learn about cations, anions, and polyatomic ions. Understand the laws of definite proportions and multiple proportions. Dive into monatomic and polyatomic ions for a comprehensive understanding of binary and ternary compounds. Master naming conventions for binary molecular compounds and common acids. Enhance your knowledge of chemistry today!

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Chemical Names and Formulas

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  1. Chemical Names and Formulas

  2. Molecules • The smallest electrically neutral unit of a substance • Oxygen

  3. Molecular Compounds • Atoms of different elements combine chemically to form compounds • Water

  4. Ions • Atoms or groups of atoms that have a positive or negative charge. • An ion forms when an atom or group of atoms loses or gains electrons

  5. Cations and Anions • Cations form ions by losing one or more electrons • Remember, electrons are negative. If you lose a negative you become more positive • Anions form ions by gaining one or more electrons • Remember, electrons are negative. If you gain a negative you become more negative

  6. Ionic Compounds • Compounds composed of cations and anions. • Cations are classified as metals and anions are classified as non-metals.

  7. Chemical Formulas • Shows kinds and numbers of atoms in the smallest representative unit of the substance • Monatomic elements are represented by their atomic symbols • If there is more than one element a subscript is used

  8. Molecular Formulas • Shows the kinds and numbers of atoms present in a molecule of a compound • Molecular formulas show the composition of the molecule but does not tell you the molecule’s structure

  9. Formula Unit • Lowest whole-number ratio of ions in a compound • NaCl 1:1 • MgCl2 1:2

  10. Law of Definite Proportions • In samples of any chemical compound, the masses of the elements are always in the same proportions • If you had 100g of magnesium sulfide and break it down into its elements, you will always obtain 43.13g of magnesium and 56.87g of sulfur

  11. Law of Multiple Proportions • Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in ration of small whole numbers • H2O O 1 • H2O2 O 2

  12. Monatomic Ions

  13. Classic Names of Monatomic Ions • Copper (I) Cuprous • Copper (II) Cupric • Iron (II) Ferrous • Iron (III) Ferric • Lead (II) Plumbous • Lead (IV) Plumbic • Tin (II) Stannous • Tin (IV) Stannic

  14. Polyatomic Ions • -ite endings have 1 less oxygen atoms than the –ate endings

  15. Binary Compounds • Compounds composed of two elements. • Cation goes first • Anion is second with the ending replaced with –ide • Overall charge must be zero

  16. Ternary Compounds • Compound that contains atoms of three different elements • Usually contain a polyatomic ion

  17. Binary Molecular Compounds • Composed of two nonmetallic compounds • Use prefixes to tell how many atoms are in the compound • Mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-

  18. Naming Common Acids

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