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Standard 1 Atomic Structure Chapters 4-6. Nobel gases halogens Semi-metals Transition metals Alkaline earth metals Alkali metals Metal/non-metal boundary.

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Presentation on theme: "Standard 1 Atomic Structure Chapters 4-6. Nobel gases halogens Semi-metals Transition metals Alkaline earth metals Alkali metals Metal/non-metal boundary."— Presentation transcript:

1 Standard 1 Atomic Structure Chapters 4-6

2 Nobel gases halogens Semi-metals Transition metals Alkaline earth metals Alkali metals Metal/non-metal boundary. Metals Non-metals Periodic Table.

3 Summary 1 Which elements are semi-metals?

4 Metals: –Good conductors –Solid (except mercury) –Lose electrons –Example = aluminum Semi-metals (metalloids): –Have properties of both metals and non-metals –Common use = –semi-conductors –Example = silicon 1b: groups of the Periodic Table Non-metals: –poor conductors –Mostly liquid/gas –gain electrons –Example = nitrogen Halogens: –Extremely reactive –Gain 1 electron –Mostly gases –Example = fluorine

5 Summary 2 1.Describe the differences between metals and non-metals. 2.Give an example of a metal 3.Give an example of a non-metal

6 1c: Periodic Groups Alkali metals –Extremely reactive –Lose 1 electron –Example: sodium Alkaline earth metals –Reactive –Lose 2 electrons –Example: calcium Transition metals –Can lose different numbers of electrons –Example: copper Noble gases –Extremely un- reactive –Gases! –Example: helium

7 Summary 3 Which group of metals are most reactive?

8 The Periodic Table: organizes elements in groups and periods. Groups/families: elements have the same physical and chemical properties. Rows/periods: elements have the same number of electron shells. 1a: organization of the periodic table

9 Summary 4 1.Name another element that would have similar chemical properties to chlorine. 2.Name an atom that is in the same period as chlorine.

10 The Periodic Table: organizes elements according to atomic number Atomic number = number of protons C Atomic number

11 Mass Mass number: the number of protons and neutrons in an atom (units = amu) Atomic mass (shown on the periodic table): the average mass of all isotopes Isotope: an atom with the same number of protons and a different number of neutrons Note: atomic mass generally increases across the periodic table but not always… (look at atomic number 27&28, 52&53)

12 Isotopes ex:

13 Summary 5 1.What is the mass number for each isotope of neon shown in the example? 2.What is the atomic mass for neon?

14 Standard 1d: electrons All atoms have an equal number of protons and electrons –Atoms are electrically neutral Atoms have no charge Symbol: Ne An equal number of positive protons and negative electrons results in zero charge

15 Summary 6 How many electrons are in a magnesium atom?

16 When an atom gains or loses electrons it becomes an ion –Ion = charged particle number electrons number protons NaNa + symbol

17 Summary 7 If a magnesium atom loses two electrons, how many electrons will this magnesium ion have?

18 1 valence e - 4 valence e - Valence electrons are: responsible for chemical behavior of atom used for chemical bonding located in the outer orbital

19 Summary 8 1.How many valence electrons does nitrogen have? 2.How many total electrons does nitrogen have?

20 Identifying Atoms by Emission Spectrum: Adding energy excites electrons. Electrons release energy when they return to the ground state (lowest energy level) Released energy = emission spectrum Each atom has a unique emission spectrum Scientists use this information in many ways: CSI can identify elements in an unknown sample Astronomers can identify elements in stars across the universe

21 Summary 9 What causes an emission spectrum?

22 Electronegativity: The ability of an atom to attract an electron Example: chlorine is very electronegative because it wants to ______ an electron. Example: sodium is not very electronegative because it wants to ______ an electron. 1c: Periodic Trends

23 General trend for electronegativity: Increasing electronegativity Increasing Note: for noble gases electronegativity = zero

24 Summary 10 1.Which is more electronegative: iodine or chlorine? 2.Which is more electronegative: argon or chlorine?

25 Ionization energy: the energy needed to remove an electron from an atom Example: fluorine has a high ionization energy because it wants to ______ an electron. Example: potassium has a low ionization energy because it wants to ______ an electron.

26 General trend for ionization energy: Increasing ionization energy Increasing Note: noble gases have a high ionization energy

27 Summary 11 1.Which has a higher ionization energy: iodine or chlorine? 2.Which has a higher ionization energy: argon or chlorine? 3.Which has a lower ionization energy: chlorine or magnesium?

28 General trend for atomic size (volume) Decreasing atomic size Increasing decreasing

29 Summary 12 Which is larger: magnesium or calcium? Which is larger: magnesium or chlorine?

30 General trend for ionic size. When atoms lose electrons they get much smaller When atoms gain electrons they get much larger

31 Summary 13 Why is Na + smaller than Na?

32 1.All the mass of an atom is in the nucleus (Protons & neutrons are in the nucleus) 2.In between the nucleus and the electrons there is only empty space Standard 1e: The structure of an atom

33 Summary 14 Which particles inside the atom have mass?

34 Earnest Rutherford Rutherford demonstrated that the entire atom is 10,000 times larger than the nucleus The rutherford experiment: A stream of positive particles (alpha particles) is aimed at a piece of gold foil. Only 1 in 8000 particles is deflected (pass close to the gold nucleus). All other particles travel through empty space

35 Summary 15 How does Rutherfords experiment demonstrate that an atom is mostly empty space?


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