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Chemistry 1d - Students know how to use the periodic table to determine the number of electrons available for bonding.

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Presentation on theme: "Chemistry 1d - Students know how to use the periodic table to determine the number of electrons available for bonding."— Presentation transcript:

1 Chemistry 1d - Students know how to use the periodic table to determine the number of electrons available for bonding.

2 How to identify an element: - Look at the protons How to find protons: -Look at the atomic number How to find neutrons: -Subtract atomic mass from atomic number (the # of protons) How to find electrons in a neutral (no charge) atom : - Always equals the number of protons

3 Atomic number tells us how many electrons an atom has in a neutral atom Valence electrons (the outermost e-) are known by looking at the elements’ family/group

4 Arrangement of the periodic table which tells us where each electron in an atom is located (which energy level and sublevel) and explains how electrons fill an atom - Nucleus Which Orbital do I go to? Negative electron

5 Energy Levels Rows/Periods = Energy Levels (7 on PT) Energy levels are divided into sublevels (s, p, d, f) Sublevels are divided into a shape of space called orbitals Each orbital/shape can ONLY hold 2 electrons!

6 The periodic table can be divided into sections called blocks (energy sublevels) 4 blocks/sublevels = s, p, d, f s, p, d, f sublevels are divided into orbitals s = 1 shape p = 3 shapes d = 5 shapes f = 7 shapes

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8 Remember…S, P, D, & F blocks refer to the shape of the orbital in which electrons are found!

9 Helium is moved over by Hydrogen

10 How many electrons can fit in each Orbital? Just Count the # of Elements in each Block!

11 2 ELECTRONS 6 Electrons 10 Electrons 14 Electrons

12 s-block = 2 electrons p-block = 6 electrons d-block = 10 electrons f-block = 14 electrons

13 1.N = 1 (1 st row/energy level): Smallest energy level Can only hold 2 electrons (2 = s-block) 2.N = 2 (2 nd row/energy level): A little larger than the first Can only hold 8 electrons (2 = s-block; 6 = p- block)

14 3.N = 3 (3 rd row/energy level): A little larger than the second Can hold 18 electrons (2 = s-Block; 6 = p-Block; 10 = d-Block) 4.N = 4 (4 th row/energy level): Larger than the third energy level Can hold 32 electrons 5.N = 5 (5 th row/energy level): Larger than the fourth energy level Can hold 50 electrons

15 6.N = 6 (6 th row/energy level): Larger than the 5th energy level Can hold 72 electrons 7.N = 7 (7 th row/energy level): Largest energy level Can hold 98 electrons

16 s p d f 1S 2S 3S 4S 5S 6S 7S 4F 5F 3D 4D 5D 6D 2P 3P 4P 5P 6P 7P The S-Block always fills first! D-Block ONE Row Behind! F-Block TWO Rows Behind!

17 1s 2s 3s 4s 5s 2p 3p 3d 4p 4d 5p 6s5d 6p 4f 7s6d 7p 5f

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19 1 2 3 4 5 6 7 s d p f

20 1.Find the element. 2.List the energy levels, orbitals (blocks), and number of electrons in each block as you make your way to the element that you are trying to find the configuration for. Cerium 1s 2 2s 2 p 6 3s 2 p 6 d 10 4s 2 p 6 d 10 f 1 5s 2 p 6 d 1 6s 2

21 1 2 3 4 5 6 7 s d p f He 1s 2 What is the Atomic Number of Helium?

22 1 2 3 4 5 6 7 s d p f Cl 1s 2 2s 2 2p 6 3s 2 3p 5

23 Energy Levels

24 1s 2 2s 2 2p 6 3s 2 3p 5 Orbitals

25 1s 2 2s 2 2p 6 3s 2 3p 5 Electrons Check work by counting number of electrons!

26 For this presentation, the nucleus of the atom is at the center of the three axes. x y z

27 The “1s” orbital is a sphere, centered around the nucleus

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30 The 2s orbital is also a sphere.

31 The 2s electrons have a higher energy than the 1s electrons. Therefore, the 2s electrons are generally more distant from the nucleus, making the 2s orbital larger than the 1s orbital.

32 1s orbital

33 2s orbital

34 2p x x y z

35 2p x and 2p z x y z

36 The three 2p orbitals, 2p x, 2p y, 2p z x y z

37 once the 1s orbital is filled,

38 the 2s orbital begins to fill

39 once the 2s orbital is filled,

40 the 2p orbitals begin to fill

41 each 2p orbital intersects the 2s orbital and the 1s orbital

42 each 2p orbital gets one electron before pairing begins

43 once each 2p orbital is filled with a pair of electrons, then

44 the 3s orbital gets the next two electrons

45 the 3s electrons have a higher energy than 1s, 2s, or 2p electrons,

46 so 3s electrons are generally found further from the nucleus than 1s, 2s, or 2p electrons

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