Organization of The Periodic Table. Open Chemical Building Blocks Book to Page 85. Get chalkboards, chalk, and eraser

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1 Organization of The Periodic Table Open Chemical Building Blocks Book to Page 85. Get chalkboards, chalk, and eraser

2 Nucleus Center of the atom. Makes majority of the atom s mass. Made of Protons and Neutrons. Nucleus

3 Protons Part of the nucleus Have positive (+) charge

4 Neutrons Part of the nucleus Have neutral charge

5 Electrons Orbit around the nucleus Have negative (-) charge

6 Atomic Number Definition: the number of protons in the nucleus Tells us the identity of the element. Every element is defined by the number of protons in its nucleus

7 Isotopes Atoms with the same number of protons but different numbers on neutrons Example: Carbon So you can change the number of neutrons and the element still maintains its identity

8 Questions 1) What particles make up an atom? 2) What are the charges on these particles? 3) What particles make up the nucleus?

9 Questions 1) What is Oxygen s atomic number? 2) How many protons does Oxygen have? 3) If I have 4 protons what element am I? 4) If I have 4 neutrons what element am I?

10 Reading the Periodic Table Mass

11 Atomic Mass Definition: the ~ mass of one atom of an element Tells us how much one atom weighs in atomic mass units. Mass

12 Organization of The Periodic Table Group/Family Period Ordered by atomic mass. Columns arranged to form groups with similar properties

13 Assessment Which element has the greatest atomic mass? Lithium Sodium Potassium Rubidium

14 The ease and speed with which an element combines, or reacts, with other elements or compounds Reactivity Pure sodium reacts explosively with air

15 Groups/families of elements have similar reactivity Group 1: metals that react violently with water Group 18: Gases that barely react at all Why do groups/families of elements react the same way?

16 Atoms have neutral charge # of Protons (+) = # of Electrons (-) = 0 charge Example: Hydrogen How many electrons does C have?

17 Electrons orbit in shells 1 st shell can fit 2 electrons 1 st period/row 2 nd and 3 rd shells can fit 8 electrons 2 nd period/row 3 rd period/row

18 Atoms want their shells to be full 2 electrons in first shell 8 electrons in 2 nd and 3 rd shells Examples:

19 Question How many electrons does an oxygen have? How many electrons are in its outer shell? Which group is oxygen most likely to react with?

20 Question For the first 3 periods: 1) How many electrons are in the outer shell of each element in group 1? Group 2? Group 13? Group 14? Group 15? Group 16? Group 17? Group 18? 2) How many electrons does each element in each group above need to fill its outer shell? 3) Which groups are the most likely to react with one another? 4) Which group is least likely to react with any other group?

21 Only use the 1 st 3 periods For the first 3 periods: 1) How many electrons are in the outer shell of each element in group 1? Group 2? Group 13? Group 14? Group 15? Group 16? Group 17? Group 18? 2) How many electrons does each element in each group above need to fill its outer shell? 3) Which groups are the most likely to react with one another? 4) Which group is least likely to react with any other group?

22 Take home message The properties of an element can be predicted from its location on the Periodic Table This is largely a result of the number of electrons in their outer shell.

23 Metals, Metalloids, and Nonmetals

24 Shiny Solids (at room temp) Malleable can be hammered flat Ductile can be pulled into wire High Conductivity ability to transfer heat or electricity to another object Metals

25 Reactivity of Metals High Low Metals will usually lose electrons when they react with other elements

26 Nonmetals Opposite of properties of metals Not shiny Poor conductors Mostly gases (at room temperature) Solids are brittle Sulfur

27 Reactivity of Nonmetals Low High Low Nonmetals will usually gain or share electrons when they react with other elements

28 Some Important Nonmetals Carbon important element for making up living organisms Noble Gases group 18 very nonreactive. Have full outer shells.

29 Inbetween metals and nonmetals Solids (at room temp) brittle and hard Semiconductors can conduct electricity under some conditions but not others. very important for computer chips Most common example Silicon in sand and glass Metalloids

30 Assessment The atomic number is the number of valence electrons. neutrons. protons in the nucleus. electrons in the nucleus.

31 Assessment The periodic table is a chart of the elements that shows the repeating pattern of their energies. properties. element symbols. names.

32 Assessment Which piece of information cannot be found in a square on the periodic table? Atomic mass. Chemical symbol. Atomic number. Number of neutrons.

33 Assessment Which element will have properties most similar to Calcium? Potassium. Scandium. Magnesium. Bromine.

34 Assessment Which group is most likely to lose/share 2 electrons in a chemical reaction?

35 Assessment Which side of the periodic table contains most of the nonmetals? Left side. Right side. Middle.

36 Assessment Which is not a property of nonmetals? Brittle. Nonmalleable. High conductivity. Most are gases at room temperature

37 Assessment Which metal is probably the most reactive? Potassium Calcium Scandium Titanium

38 Assessment Which nonmetal is probably the most reactive? Nitrogen Oxygen Fluorine Neon