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Atoms, Molecules, and Ions

This resource provides an overview of fundamental concepts in chemistry, focusing on atoms, molecules, and ions. It highlights the contributions of notable scientists such as Dalton, Thomson, Millikan, Rutherford, and Chadwick. Key topics include atomic structure, types of chemical bonds (ionic and covalent), the periodic table's organization, and the naming conventions for ionic and covalent compounds. Understanding these concepts is essential for grasping the basics of chemistry and the behavior of matter at the atomic level.

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Atoms, Molecules, and Ions

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  1. Atoms, Molecules, and Ions

  2. Important Scientists • Greeks fire, earth, wind, water • Dalton father of atom; sphere • Thomson cathode ray tube; charged particles • Millikan mass of electron; oil drop experiment • Rutherford nucleus; gold foil experiment • Chadwick missing mass; neutron

  3. The atom symbol/chargemass (kg) mass (amu) location proton p+ 9.11 X 10-31 kg 1 amu nucleus neutron n0 1.67 X 10-27 kg 1 amu electron e- 1.67 X 10-27 kg 0 energy levels

  4. Need to know Atomic number = # protons Mass number = # protons + # neutrons Atomic mass or weight = weighted average of all isotopes of an element Isotope = atom of an element with same atomic number but different mass number mass # 6529Cu copper-65 atomic #

  5. Chemical formulasDepend on type of bond Ionic bonds • Write symbols • Check charges • Crisscross charges if necessary • Parentheses around polyatomic ions ex. Magnesium phosphate Mg2+ PO43- Mg3(PO4)2

  6. Covalent bonds Prefixes tell how many of each element No charges involved mono- 1 di- 2 ex. trioxygen tetrafluoride tri- 3 O3F4 tetra- 4 penta- 5 hexa- 6 phosphorus pentachloride hepta- 7 PCl5 octa- 8 nona- 9 deca- 10

  7. Ions Formed when atoms lose or gain electrons Lose or gain to follow octet rule (filled valence level) Lose form cation Mg 12 p+ Mg2+12 p+ positive charge 12 e- 10 e- Gain form anion S 16 p+ S2- 16 p+ negative charge16 e- 18 e- (atom) (ion) (atom) (ion)

  8. GroupsVertical columns special names valence e- ion Group IA alkali metals 1 e- Na+ IIA alkaline earth metals 2e- Mg2+ IIIA aluminum group 3 e- Al3+ VA nitrogen group 5e- N3- VIA oxygen or chalcogen 6e- O2- VIIA halogens 7e- F- VIIIA noble or inert gases 8e- Ne

  9. Periods Horizontal rows Tell how many energy levels contain electrons ex. period 3 has electrons in 3 energy levels period 6 has electrons in 6 energy levels

  10. Parts of periodic table Metals/nonmetals Metals to left of stair step line Nonmetals to right of stair step line [Metalloids touch either side of stair step line] representative elements group ‘A’ elements transition elements group ‘B’ elements inner transition elements bottom 2 rows

  11. Naming ionic compounds • name cation + name anion • -ide ending if anion is single element • Roman numerals for transition elements if needed. ex. CaCO3 calcium carbonate FeCl3 iron (III) chloride

  12. Naming covalent compounds • name first element + name second element • -ide ending on last element only • prefixes to tell how many of each ex. CCl4 carbon tetrachloride (mono- is never used on the first element) CO carbon monoxide

  13. Naming Acids no oxygen hydro- + -ic -ate -ic to root name -ite -ous to root name ex. Acid anion name HCl chloride hydrochloric acid HClO4 perchlorate perchloric acid HClO3 chlorate chloric acid HClO2 chlorite chlorous acid HClO hypochlorite hypochlorous acid

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