Chapter 11 The Chemical Elements

Transcription

1 James T. Shipman Jerry D. Wilson Charles A. Higgins, Jr. Omar Torres Chapter 11 The Chemical Elements

2 Chemical Classification of Matter Mass and Volume H 2 O, sugar, O 2, Fe H, Cu, Fe CO 2, H 2 O..

3 Which of these is a pure substance? Sugar Ice Baking Soda

4 The Periodic Table Elements are arranged in the order of increasing atomic number. Divided into 7 periods and 18 groups Section 11.4

5 Classification of the Periodic Table Alkali Metal Alkali Earth Metal Period Group Halogen Noble Gas

6 Shapes of atomic orbitals S orbital z y x

7 Shapes of atomic orbitals p orbital

8 Shapes of atomic orbitals d orbital

9 Shapes of atomic orbitals f orbital

10 Electron Configurations: How the electrons are distributed in an atom. 1s 1s 2s 3s 4s 5s 6s 7s 3d 4d 5d 6d 2p 3p 4p 5p 6p 7p 4f 5f

11 Hydrogen Electron Configuration Periodic number 1 Number of electrons Block designation

12 Helium Electron Configuration 2

13 Lithium Electron Configuration 1s 2 2s 1

14 Boron Electron Configuration 1s 2 2s 2 2p 1

15 Oxygen Electron Configuration 1s 2 2s 2 2p 4

16 Atomic Size Atomic size is estimated as 1/2 the distance between the centers of two bonded atoms.

17 Trends in Atomic Size

18 Trends in Atomic Size

19 Valence electrons. Valence electrons: are the outermost electrons in an atom Valence electrons equal to group number

20 Ionization Energy the energy required to remove a valence electron from a gaseous atom to form a gaseous ion.

21 Periodic trends Ionization Energy

22 Ionic Size The radius of Na + is smaller than Na

23 Ionic Size The radius of Cl - is larger than Cl

24 Seven Common Elements that Exist as Diatomic Molecules These atoms (H, N, O, F, Cl, Br, I) are too reactive to exist as independent atoms When writing formulas w/ these seven elements we us the diatomic form: H 2 +Cl 2 2HCl Section 11.3

25 Eleven Compounds with Special Names Section 11.5

26 Naming a Binary Compound for a Metal and Nonmetal Binary = two-element compound First give the name of the metal and then give the name of the nonmetal, changing its ending to ide NaCl sodium chloride Al 2 O 3 aluminum oxide Ca 3 N 2 calcium nitride Section 11.5

27 Section 11.5

28 Compounds of Two Nonmetals The more metallic or less nonmetallic element (farther left or farther down periodic chart) is usually written first in the formula and named first The second element is named using the ide ending Greek prefixes are used to designate the number of atoms in the molecule Section 11.5

29 Examples: HCl hydrogen chloride CS 2 carbon disulfide PBr 3 phosphorus tribromide IF 7 iodine heptafluoride Section 11.5

30 Polyatomic Ions Ion an atom or chemical combination of atoms having a net electric charge Monatomic ion an ion formed from a single atom (Cl ) Polyatomic ion an electrically charged combination of atoms (CO 3 2 ) Name the metal and then the polyatomic ion: ZnSO 4 zinc sulfate NaC 2 H 3 O 2 sodium acetate Mg(NO 3 ) 2 magnesium nitrate K 3 PO 4 potassium phosphate Section 11.5

31 Common Polyatomic Ions Section 11.5

32 Acids When Hydrogen (H) Is Combined with Polyatomic Ions Section 11.5

33 Naming Compounds Example H 2 SO 4 sulfuric acid (special name) ZnCO 3 zinc carbonate (metal + polyatomic ion) Na 2 S sodium sulfide (binary compound of metal + nonmetal) SiO 2 silicon dioxide (binary compound of two non-metals) NH 3 ammonia (special name) NH 4 NO 3 ammonium nitrate (ammonium ion + polyatomic ion) Section 11.5

34 Homework Exercises