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Atomic Review and Naming Compounds

Atomic Review and Naming Compounds. Electron (e - ) orbit/energylevel. Proton (p + ). nucleus. Neutron (n 0 ). # of p +. p + + n 0. Atoms that have the same number of protons but a different number of neutrons are called Isotopes. Hydrogen Atomic Mass = 1 Atomic Number = 1.

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Atomic Review and Naming Compounds

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  1. Atomic Review and Naming Compounds

  2. Electron (e-) orbit/energylevel Proton (p+) nucleus Neutron (n0)

  3. # of p+ p+ + n0

  4. Atoms that have the same number of protons but a different number of neutrons are called Isotopes. Hydrogen Atomic Mass = 1 Atomic Number = 1 Deuterium Atomic Mass = 2 Atomic Number = 1

  5. Atoms can either gain or lose electrons Gain - negatively charged ion. Loses - positively charged ion H : neutral atom H+ : positive ion H- : negative ion

  6. Octet rule: atoms react to acquire a full outer shell: • Give away an e- to another atom. • Take an e- from another atom. • Share an e-with another atom. Ionic bond Covalent bond An ION is an atom that has lost or gained an electron. Lose e- – positive ion OR cation. (metals) Gain e- – negative ion OR anion. (nonmetals)

  7. +1 +3 -3 -2 -1 +2 +4/-4 Remember: The number of the column is equal to the valence electron number. Know that and you figure out the number of electrons lost or gained – the ionic charge

  8. Ionic NaCl Covalent HCl A compound has different characteristic properties than the atoms which form it.

  9. Diatomic Elements: Elements that are most commonly found in a covalent bond with itself. I Have No Bright Or Clever Friends I2H2N2Br2 O2Cl2F2

  10. Chemical formula gives the following information: · The different elements in the compound. · The numberof atoms in the compound.

  11. Writing Rule 1: Write the symbol of the metallic element first. Beryllium combines with Chlorine + 2 - 1 Be Cl Rule 2: Place the combiningcapacityof one element as a subscript of the other element.

  12. Rule 3:Leave subscripts with a value of 1 out. Be Cl2 1 • Two Naming rules: • Write the full name of the metal ionfirst. • Name the non-metal iondropping the last • part of the name and adding the suffix “ide”. beryllium chlor ide

  13. Rule 4: Reduce the subscripts if possible. Magnesium combines with Sulfur + 2 - 2 Mg S MgS magnesium sulph ide

  14. Transition metals

  15. Transition metals can give away different numbers of electrons. To avoid confusion: Brackets are used to show how many electrons the Transition metal is giving away.

  16. Iron (II) chloride Iron (III) chloride + 2 - + 3 - 1 1 Fe Cl Fe Cl FeCl2 FeCl3

  17. Write the name of the ionic compound: +4 -2 Remember: Always look at the anion to see if it has been reduced. If it has, so has the metal. - + Pb O PbO 2 1 lead oxide (IV)

  18. Covalent Compound: Contain two or more NON-METAL atoms. Formed by SHARING valence electrons to fill outer shell – octet rule. • A molecule is the smallest unit of a covalent compound. Non-metal + Non-metal = covalent bonding

  19. Step 1: firstnon-metal is named with a prefix to show the number of atoms. We do not use “mono” for the first non-metal. Step 2: secondnon-metal is named with a prefix AND with the “ide” ending. N O 2 4 nitrogen oxide di tetra dinitrogen tetroxide

  20. Writing formulas Step 1: Write the symbol of each element. Step 2: Use a subscriptto show the number of each type of atom given by the prefix. Do not reducecovalent formulas. di phosphorus oxide penta PO 2 5

  21. Does it have a metal? YES Is it a transition? NO • NO charges • NO criss-cross • Use prefixs • Ends in “ide” • NO • Find charges • Criss-cross • Ends in “ide” • YES • Find charges • Reverse Criss-cross • Use Brackets • Ends in “ide”

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