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FAMILIES OF ELEMENTS

FAMILIES OF ELEMENTS. Groups/Families. Group 1: ALKALI METALS Group 2: ALKALINE EARTH METALS Group 3-12: TRANSITION METALS (Inner transition metals- rare earth elements) Groups 13-18: NON-METALS (mostly) Group 17: HALOGENS Group 18: NOBLE GASES.

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FAMILIES OF ELEMENTS

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  1. FAMILIES OF ELEMENTS

  2. Groups/Families Group 1: ALKALI METALS Group 2: ALKALINE EARTH METALS Group 3-12: TRANSITION METALS (Inner transition metals- rare earth elements) Groups 13-18:NON-METALS (mostly) Group 17: HALOGENS Group 18:NOBLE GASES

  3. The periodic table contains all the known elements in order of increasing atomic number. • Elements of atoms with similar structures have similar properties. Therefore, they are positioned close to each other. • Elements can be divided into metals and nonmetals forming large groups.

  4. There is consistencyin chemical properties of the elements. This happens because the electrons in atoms are arranged in shells. • Each shell holds a certain number of electrons. • All elements with the same numberof electrons in the outermost shell behave in similar ways. (Same GROUPS) • Elements will combine with other elements in order to complete/fill their outer shells. When elements combine, (usually a metal & nonmetal) a compound is formed.

  5. These are diagrams that show energy levels for electrons surrounding the nucleus of a particular atom. EXAMPLE: LITHIUM Electron Configurations • 3 Li 6.941 3P 4N 3P 4N • 2 1 Li OR • Bohr (Shells) Dot diagram Element box Bohr Model

  6. Circle your level of understanding of these concepts: 1 2 3 4

  7. Metals • Most of the elements are classified as metals • Metals usually have 3 or less electronsin their outer energy level. Therefore, metals give away electrons (or lose e-) when forming compounds • They usually have a lusterorshine • Most metals are good conductorsof heat and electricity • They are malleableandductile

  8. These elements: • contain oneelectron in their outer energy levels. • are the most chemically active of all the metals. They are so close to having a full shell that they want to bond with other elements and lose that electron; this makes them very reactive metals. • Most compounds are white. Ex: Table salt Alkali Metals: Group IA (1) (except hydrogen)

  9. These elements: • are shiny, good conductors, malleable, and light weight. • are never found in pure form in nature. • react violently with oxygen and water. Which is why these metals are stored covered in oil. Alkali Metals: Group IA (1) (except hydrogen)

  10. Alkaline Earth Metals: Group IIA (2) These elements: • contain two electrons in their outer energy levels. • are the 2nd most reactive metals. • They form compounds by losing electrons. Some react with water.

  11. Alkaline Earth Metals: Group IIA (2) These elements: • have the same metallic properties as the alkali metals, but are slightly less reactive. • Magnesium and calcium are most common compounds found in nature (animals & plants).

  12. These elements: have a lot of electrons and distribute them in different ways than the other elements. are able to put up to 32 electrons in their second-to-last shell.  contain one or two electrons in their outer (last) energy levels. Transition Metals: Groups III – XIIB (3-12)

  13. Transition Metals: Groups III – XIIB (3-12) These elements: can lose one or bothof these electrons. can use the two outermost shells/orbital to bond with other elements.They can also share electrons when forming compounds.

  14. Transition Metals: Groups III – XIIB (3-12) have low ion charges. are usually colored. are great conductors, very hard, malleable, and shiny with high melting and boiling points. form alloysthat are mixtures composed of 2 or more metals or a metal and a nonmetal.

  15. Circle your level of understanding of these concepts: 1 2 3 4

  16. Non-Metals • Non-metals tend to vary more from element to element. • Non-Metals usually have 5 or more electronsin their outer energy level. Therefore, non-metals stealelectrons (or gain e-) when forming compounds • They usually gases at room temp. • The few solids are dull & brittle • Non-metals are poor conductors of heat and electricity

  17. Group XVIIA (17): Halogens These elements: • contain seven electrons in their outer energy levels. • form compounds by gaining an electron. • have the trait of combining with many different elements since they are only missing one electron. Bond with metals and element in Group 1. • are reactive. Fluorine is the most reactive, and then it decreases as you go down.

  18. These elements: contain eight electrons in their outer energy levels. last energy levels are full so they usually do not bond with other elements, especially in nature. are nonreactive. become more rare as you move down the group. Group XVIII (18): Noble Gases

  19. Circle your level of understanding of these concepts: 1 2 3 4

  20. Synthetic Elements • Elements with atomic numbers 43, 61, 93 and above are syntheticelements. • They are produced in nuclear reactions. • All of these elements breakdown into other elements.

  21. Alloys have properties that pure metals composing them do not have. Example: • An alloy of iron and chromium does not rust, but iron does. • Steel is an alloy composed mainly of iron and carbon. Alloys

  22. Circle your level of understanding of these concepts: 1 2 3 4

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