Physical Science 9 The Periodic Table

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1 Physical Science 9 The Periodic Table 0801 Chapter 3.2 1

2 Physical Science 9 The Periodic Table 0801 Chapter 3.2 2

3 Physical Science 9 Atomic Structure The Periodic Table groups elements together much like a grocery store groups items in the same aisle. Where is the Malt-O- Meal you rebel scum! 0801 Chapter 3.2 3

4 2: Chapter 3.2 4

5 Physical Science 9 Simplified Periodic Table See pages in your text 0801 Chapter 3.2 5

6 Periodic Table with electron configurations 0801 Chapter 3.2 6

7 Standard Periodic Table 0801 Chapter 3.2 7

8 1: Chapter 3.2 8

9 Standard Periodic Table 0801 Chapter 3.2 9

10 Standard Periodic Table Symbol A one or two letter abbreviation for an element. The first letter is ALWAYS upper case. Atomic Number The number of protons in the atom. The periodic table is arranged in proton order from left to right. Element name The name of the element. Atomic Mass The number of grams of one mole of the element (mass of the element). Elements that have more protons generally have more mass, therefore mass increases as you move from left to right Chapter

11 Standard Periodic Table You do NOT have to memorize data in the Periodic Table. It will ALWAYS be available to you for tests and homework. The Periodic Table is your FRIEND!!! 0801 Chapter

12 Physical Science 9 Other Periodic Tables 0801 Chapter

13 Physical Science 9 Other Periodic Tables 0801 Chapter

The Periodic Table of the Elements Created by an old Russian guy named Dmitri Mendeleev in 1869.

14 The Periodic Table of the Elements Created by an old Russian guy named Dmitri Mendeleev in He arranged the known elements of his day in a table with each column representing elements that had similar chemical properties Chapter

15 The Periodic Table of the Elements I was a genius of my time, and I also had many, many bad hair days. His original table included spaces for elements that had not been discovered yet Chapter

16 The Periodic Table of the Elements Mendeleev s Table had some problems, but they pretty much eliminated when his table was modified to list elements according to atomic mass Chapter

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18 The Periodic Table According to your book, there are 92 naturally occurring elements. However, only 88 have actually been found in nature. The others have been synthesized in labs or in atomic reactions. Uranium (U, atomic number 92) is the heaviest naturally occurring element. All of the heavier elements were created in labs by shooting a stable atom with protons hoping one will stick. Some of these atoms exist only for nanoseconds before the extra proton is dumped Chapter

19 Physical Science 9 Electron Configuration The electron configuration of an atom is a form of notation which shows how the electrons are distributed among the various atomic orbital and energy levels. Orbitals are filled in a certain order. Energy levels are not filled one at a time many times the higher energy orbitals (d and f) are skipped Chapter

20 Physical Science 9 Electron Configuration Example Hydrogen has 1 electron. Using the chart below, it is easy to see that the 1s orbital would be used to store this one electron. Therefore, hydrogen s electron configuration would be 1s 1 The first letter exponent number is the is orbital the is the number that energy the of level electrons of the is held in. atom in where that orbital. the electron is Chapter

21 Physical Science 9 Electron Configuration How about Helium? It has two electrons in each atom. The electron configuration for Helium would be 1s Chapter

22 Physical Science 9 Electron Configuration What about Oxygen? It has eight electrons in each atom. The electron configuration for Oxygen would be 1s 2 2s 2 2p 4 If you add up all the exponents, it should equal the number of electrons 0801 Chapter

23 Physical Science 9 Electron Configuration Let s blow you away with a tough one. Let s write the electron configuration of Krypton. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p Chapter

24 Physical Science 9 Electron Configuration 0801 Chapter

25 0801 Chapter

26 0801 Chapter

27 Physical Science 9 Electron Configuration Using the Periodic Table to do electron configurations 0801 Chapter

28 Physical Science 9 Electron Configuration Shortcut Using Noble Gases 0801 Chapter

29 0801 Chapter

30 Physical Science 9 Ions vs. Atoms All atoms have a common goal It is the same goal that many of us have We want to have a fulfilling life Atoms want to be full as well It is each atoms goal to acquire EIGHT (8) electrons in its outer energy level (there are a few exceptions which we ll cover later.) 0801 Chapter

31 Physical Science 9 Ions vs. Atoms As you remember from a previous discussion, the outer energy level electrons are called valence electrons. As it turns out, the closer an atom is to having eight valence electrons the more effort it has to attain that goal. Those atoms that are just one away from eight will do almost anything to gain another electron stealing is their way of life pillaging is their MO (modus operandi) 0801 Chapter

Along comes a sodium atom. The sodium atom has only one valence electron.

32 Physical Science 9 Ions vs. Atoms A chlorine atom has 7 electrons, and is searching for one more to take from someone. Along comes a sodium atom. The sodium atom has only one valence electron. If it could get rid of it, it would then have 8 valence electrons! Sodium wants to get rid of that one electron as much as Chlorine wants to gain one, so Sodium easily gives it up and both atoms are happy! However, they are not atoms anymore 0801 Chapter

Physical Science 9 Ions vs. Atoms Since the Chlorine atom has added an electron, it has also added an additional negative charge (remember, electrons are negative).

33 Physical Science 9 Ions vs. Atoms Since the Chlorine atom has added an electron, it has also added an additional negative charge (remember, electrons are negative). So now the atom is not electrically neutral anymore it has been ionized! It is now an ion! Since the Chlorine atom gained one negative charge, it s overall charge is -1. The Sodium atom has given up an electron, so its overall charge is +1. This charge is called the VALENCE of an ion Chapter

34 Physical Science 9 Ions vs. Atoms If an atom GAINS electrons, it becomes NEGATIVELY charged If an atom LOSES electrons, it becomes POSITIVELY charged Chapter

35 Physical Science 9 Ions vs. Atoms If an atom LOSES electrons, it becomes POSITIVELY charged these ions are called CATIONS 0801 Chapter

36 Physical Science 9 Ions vs. Atoms If an atom GAINS electrons, it becomes NEGATIVELY charged. These ions are called anions 0801 Chapter

37 Physical Science 9 Octet Rule Exceptions Hydrogen, Helium, Lithium, and Beryllium (the first four elements) are happy with two valence electrons, since the first energy level can only hold two electrons, so it s full! 0801 Chapter

38 Atomic number vs. Mass number The ATOMIC NUMBER is the number of protons in the atom. The mass number is the number of protons and neutrons in the nucleus. The mass number of an atom can vary depending on the number of neutrons. Atoms of almost any element can have different number of neutrons Chapter

39 Atomic number vs. Mass number Carbon, for instance, can commonly have 6, 7 or 8 neutrons in each atom. They would be referred to as C-12, C-13 or C Chapter

40 Atomic number vs. Mass number When you look at the Periodic Table, you will notice that Carbon has an atomic mass of If all of the Carbon atoms had 6 neutrons, the atomic mass would be exactly But since there are some C-13 and C-14 atoms mixed in, it raises the atomic mass slightly Chapter

41 Atomic number vs. Mass number These variations in the number of neutrons are called ISOTOPES So, C-12, C-13, and C-14 are isotopes of Carbon Chapter

42 Calculating the number of Neutrons To calculate the number of neutrons any atom has, take the mass number and subtract the atomic number (the number of protons). C-14 has a mass number of 14, with an atomic mass of = 8 neutrons 0801 Chapter

43 Deathly Isotopes Many isotopes are harmless. The water you drink everyday contains isotopes of both hydrogen and Oxygen (H-1, H-2, O-16, O-17 and O-18. Isotopes that are radioactive (give off energy as they decay) are dangerous and can damage living cells Chapter

44 0801 Chapter

45 Mass of a Single Atom The mass of a single atom is extremely small. Units like grams, pounds, and ounces are way too big for the mass of an atom. Scientists came up with a unit that can be used with atoms. It is called the Atomic Mass Unit. It is defined as 1/12 th the mass of a Carbon-12 atom. Since Carbon-12 has 6 protons and 6 neutrons, and since electrons contribute very little to the overall mass, it can be assumed that each proton and neutron have a mass of 1 AMU Chapter

Avogadro s Number So where do the atomic masses found in the Periodic table come from? Scientists came up with a quantity unit called the moles. 1 mole = 6.

46 Avogadro s Number So where do the atomic masses found in the Periodic table come from? Scientists came up with a quantity unit called the moles. 1 mole = 6.02 x This number was named after a funny-looking Italian scientist, Lorenzo Romano Amedeo Carlo Avogadro. We call it Avogadro s number Chapter

Avogadro s Number If you take 6.02 x 10 23 atoms (1 mole) and place them on a scale, you would come up with the atomic mass. 6.02 x 10 23 is a BIG number.

47 Avogadro s Number If you take 6.02 x atoms (1 mole) and place them on a scale, you would come up with the atomic mass x is a BIG number. If you had a mole (6.02 x ) of coke cans, they would cover the entire surface of the Earth with a depth of 200 miles Chapter

48 Avogadro s Number However, when you re talking about something as small as atoms, a mole of copper atoms would fit in a tablespoon Chapter

49 That s All Folks 0801 Chapter

1 amu 1 amu 0 amu. Chapter 2 part 1.notebook September 16, Modern Atomic Theory

1 amu 1 amu 0 amu. Chapter 2 part 1.notebook September 16, Modern Atomic Theory Chapter 2 The Atom Elements are the basic substances that make up all matter. An atom is the smallest particle of an element. Average atoms are 10 10 m in diameter. If you could put 6.02 x 10 23 p + and