Atomic Bonding and Molecules. Chapter 15

Transcription

1 Atomic Bonding and Molecules Chapter 15

2 Bonding of atoms makes molecules The Formation of Ions and Ionic Bonds Types of bonds Metallic Bonds Covalent Bonds Polar Covalent Bonds Molecular Polarity and Molecular Attractions

3 Causes of bonding Atoms bond together through their electrons Electrons behave as though they are contained within a series of seven concentric shells Outer shell electrons interact with electrons of other atoms These are the VALENCE electrons

4 Maximum number of electrons in each shell is shown Inner shell fills up before next shell begins to get electrons Full shells are most stable Electron Shells

5 Full electron shells Outer electron shells of noble gases are full

6 In Class Activity 1 Draw the electron shells for the sodium atom around the chemical symbol for sodium What element has the electron structure that sodium would have if it lost one electron?

7 Sodium Ion Formation Ion: An atom that has lost or gained one or more electrons

8 Periodic table

9 Electrons shells in periodic table First three periods

10 Electron Dot Structure A notation showing only the valence electrons surrounding the atomic symbol

11 Electron dot structure pattern

12 In Class Activity 2 How are electron shell diagrams different from electron dot structure diagrams? Do they both tell you about the valence electrons? Which is easier to draw?

13 In Class Activity 3 Draw the electron dot structure for sodium and chlorine atoms What electron change do you imagine may occur so these elements bond?

14 Molecular Ions H H O + H H + Water Hydronium ion, H 3 O + Hydrogen ion Typically formed by the loss or gain of a hydrogen ion, H +

15 Ion An atom, molecule, or compound with a different number of protons and electrons More protons: positive CAT ION THE t looks like a plus sign More electrons: negative AN ION Negative has an N in the prefix Both are all one word: anion, cation

16 Lose electrons Ion formation more protons than electrons positive charge Gain electrons More electrons than protons Negative charge More than one can be lost or gained Determine by position in periodic table

17 Electron dot structure pattern

18 Typical ions formed

19 In Class Activity 4 Draw the electron dot structure for a magnesium atom in area to right What is the charge of an ion that is formed from a magnesium atom? Why does it have this sign and amount of charge?

20 Ionic Bonds Electrical force of attraction between oppositely charged ions

21 Ionic Bond Ratios Compounds form in ratios to neutralize charges

22 Question For Thought Is the change of sodium and chlorine atoms to the ionic compound sodium chloride a physical or a chemical change?

23 In Class Activity 5 Write the chemical formula for a compound made of magnesium ions, Mg 2+, and oxygen ions, O 2 Write the chemical formula for a compound made of aluminum ions, Al 3+, and oxygen ions, O 2 Write the chemical formula of the ionic compound calcium fluoride

24 Groups of atoms forming ions Polyatomic ions Bonds within group are covalent

25 Metallic Bonds Nucleus of metal atoms only weakly hold outer electrons Weak attraction allows the electrons to move from one atom to another quite freely

26 Metallic Properties Mobility of electrons results in many properties of metals Conductive electrons move freely Shiny electrons vibrate and reflect light Malleable can move with respect to one another without breaking because electrons in constant motion Alloys electrons shared between unlike types of metal atoms

27 Metallic Alloys An alloy is a mixture of metallic elements.

28 Metal Ores Few metals naturally occur as elements Gold, copper, mercury Most occur as oxides and sulfides Ionic compounds Concentrations of these are ORE

29 Covalent Bonds Atoms are held together by their mutual attraction for shared electrons There are two electrons within a single covalent bond

30 Covalent Bond Diagrams The covalent bond is represented using a straight line F F F F

31 Covalent Water The number of covalent bonds an atom can form equals its number of unpaired valence electrons

32 Covalent Ammonia The number of covalent bonds an atom can form equals its number of unpaired valence electrons

33 Covalent Methane The number of covalent bonds an atom can form equals its number of unpaired valence electrons

34 Multiple covalent bonds are possible if atom has more than one unpaired valence electron

35 Nonpolar Covalent Bonds Electrons are shared evenly when the two atoms are the same element

36 Polar Covalent Bonds Shared unevenly when the bonded atoms are different elements

37 Polar covalent bonds Closer together on the periodic table, less polar bond Further apart on the periodic table, more polar bond Molecules are called dipoles Ionic bonds are extremely polar but not covalent

38 In Class Activity 6 Rank these compounds in order from least polarity (1) to greatest polarity (4) by number below each compound PF, SF, GaF, GeF

39 Molecular Polarity

40 Molecular Attractions Electrical attractions between molecules that does not result in bonding Ions Polar molecules Non-polar molecules

41 Water and salt Ions of NaCl attract dipole of water Ion-dipole attraction

42 Dipole-dipole attraction Water and water Dipoles of water attract one another

43 Some non-polar molecules can be distorted Dipole-Induced into dipoles dipole by polar attractions molecules--oxygen and water

44 Molecules Induced can dipole-induced develop induced dipole dipoles especially attractions if they are large

45 Teflon is nonstick Because the fluorine atoms are non-polar and don t readily become induced dipoles