Chemical Bonds CH. 18: PG
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1 Chemical Bonds CH. 18: PG
2 Today s Learning Objectives How does a compound differ from the elements that make it up? What is a chemical bond? Know how to determine the number of valence electrons for elements in groups 1, 2, and Draw electron dot structures.
3 Valence Electrons (18-1) Remember NaCl? Made of Na and Cl The properties of a compound differ from the elements that make it up.
4 Valence Electrons There are just over 100 elements, yet millions of substances exist. How?
5 Valence Electrons Chemical bond The force of attraction that holds two atoms together Such as those binding NaCl or H 2 O Electrons are the key to understanding chemical bonds
6 Remember these?? Electrons drawn in energy levels First energy level can hold 2 electrons Second energy level can hold 8 electrons Third energy level can hold 18 electrons
7 Valence Electrons Only the outermost energy level is important in bonding They are the only ones available to bond! Valence electrons The electrons in the outermost energy level of an atom How many valence electrons in the drawings on the board?
8 Valence Electrons Determining # of valence electrons Method 1: Draw the atom Method 2: Use the periodic table Ignoring the transition metals: Groups 1 & 2: valence electrons = group number Groups 13-18: valence electrons = group number minus 10 Every element in a group has the same number of valence electrons!
9 Valence Electrons Electron dot diagrams Great for drawing valence electrons! Draw the symbol for the element, surrounded by one dot for each valence electron
10 Today s Learning Objectives Be able to predict the ion formed by metals in groups 1-2, and all of the nonmetals. Know how to properly write the symbol and charge for an ion. Be able to name ions.
11 Ions (18-2) The secret to chemical bonds Every atom wants to have 8 valence electrons (that is the most stable number) Exception: H, He, Li, Be & B are happy with 2 Atoms will take, lose, or share electrons to get their total of 8 valence electrons Draw Lithium, Fluorine, Neon, and Carbon (electron dot notation). Predict how many electrons they will gain, lose, or share.
12 Ions Ions Charged particles formed when the number of protons and electrons are not equal
13 Ions Forming ions: Metals lose electrons and become positive ions Ex. Na +, Mg 2+, Al 3+ Nonmetals gain electrons and become negative ions N 3-, O 2-, F -
14 Ions You can easily predict the charges of elements in groups 1, 2, and Find the element on the periodic table Determine the closest path to a noble gas, counting the elements you pass as you go Go to the right you are adding electrons, thus becoming negative Go to the left (around the back of the table) you are losing electrons, thus becoming positive
15 Ions Don t forget what is actually happening o Atoms gain or lose electrons to achieve 8 valence electrons o If the number of protons electrons, the atom becomes an ion with a positive or negative electric charge o Charge = # protons - # electrons o Practice
16 Ions Time out writing info Superscript writing above the line, indicates charge Subscript writing below the line, indicates quantity Ions written with the atomic symbol followed by the charge in superscript Ex. Na +, Mg 2+, O 2-, F -
17 Ions Ion Review: What ions are made by the following elements: Na Al N Cl S Answers: Na +, Al 3+, N 3-, Cl -, S 2-
18 Ions Naming Ions: If positive, just use the element name Complication: If it is a transition metal, it is the element name followed by the charge in parenthesis. Ex. Fe 3+ = Iron(III) If negative, add an -ide to the end of the element name Practice
19 Today s Learning Objectives Why does chemical bonding occur? List the 3 types of chemical bonds. Describe an ionic bond. Be able to determine the formula of an ionic compound.
20 Ionic Bonds and Compounds (18-3) 3 types of chemical bonds 1. Ionic bonds 2. Covalent bonds 3. Metallic bonds
21 Ionic Bonds and Compounds Ionic bond Bond made by gaining or losing electrons, between metal & nonmetal Animation
22 Ionic Bonds and Compounds Bonding of ions: Opposites attract (like magnets) Ions will continue to attract other ions until the net charge is zero Ex: Na + + Cl - NaCl Ex: Mg 2+ + Cl - + Cl - MgCl 2 The final compound always has a net charge of zero! Animation
23 Ionic Bonds and Compounds Writing formulas Always written positive ion before negative ion Subscripts indicate simplest ratio of ions to make it neutral overall Mg 2+, Br - form MgBr 2
24 Ionic Bonds and Compounds You need to balance the charges of each ion when forming the compound How many Cl - do you need to balance out one Mg 2+? Answer: 1 Mg Cl - 1 MgCl 2 Try matching Na + and N 3- Try matching Ca 2+ and P 3- Try matching Li + and F -
25 Ionic Bonds and Compounds Crossing-over technique For writing the formula made by 2 ions 1. Write the ions down (positive first) 2. Below them, write just the symbols for the elements 3. Cross over the absolute value of the charges as subscripts 4. Simplify if possible 5. Erase the number if it is 1 Try it with Magnesium and Nitrogen Try it with Potassium and Oxygen
26 Today s Learning Objectives How do you determine the oxidation number of an element? How do you write formulas for compounds (ionic and covalent)? How do you name ionic compounds?
27 Ionic Formulas & Names (18-4) If you had to go into the store room and pick out sodium hydroxide from the following chemicals, could you do it? 1) Na 2 O 2) NaH 3) NaOH 4) Na 2 O 2
28 Ionic Formulas & Names To write a formula, you need to know the elements involved and the number of electrons they gain, lose, or share to be come stable Oxidation number a positive or negative number that indicates how many electrons an atom has gained, lost, or shared to become stable
29 The number at the top of each column is the most common oxidation number of elements in that group.
30 Ionic Formulas & Names For ions, this is easy Just use the charge of the ion If the ion is a transition metal, the charge is given to you in the name of the compound in Roman numerals Ex. Iron(III) oxide
31 Ionic Formulas & Names Rules for naming compounds can get quite complicated. We ll focus only on ionic compounds for now. Binary ionic compounds Made up of two ions (one positive and one negative) Name the compound by naming the two ions!
32 Ionic Formulas & Names First, name the cation Cations positive ions just use the element s name Ex. Na + is sodium When multiple ions possible for same element, put the charge in roman numerals Ex. Cr 2+ is chromium(ii), Cr 3+ is chromium(iii)
33 Ionic Formulas & Names Second, name the anion Anions negative ions change the end of the name to -ide Ex. F - is fluoride, N 3- is nitride Ionic compounds 2 words: cation, anion
34 Ionic Formulas & Names Practice: Determine the formula and write the name of the compounds from these ions Na + and O 2- Cu 2+ and Br - Fe 3+ and O 2- Games
35 Ionic Formulas & Names Easy so far, right? Minor complication polyatomic ions Polyatomic ion an ion formed by a group of covalently bonded atoms with a charge Ex. OH - is hydroxide You don t need to memorize the list of polyatomics, but must recognize them when they appear.
36 Polyatomic ions to recognize Ion Name Ion Formula Ammonium NH + 4 Acetate C 2 H 3 O - 2 Carbonate CO 2-3 Chlorate ClO - 3 Hydroxide OH - Nitrate NO - 3 Phosphate PO 3-4 Sulfate SO 2-4
37 Ionic Formulas & Names Naming the ionic compound doesn t change Still name the cation, then the anion But writing formulas has one change If have multiple copies of the same polyatomic ion in formula, put parenthesis around them Ex. Mg(OH) 2
38 Ionic Formulas & Names Give it a try: Polyatomic ions Ionic compounds with polyatomics Practice Naming: Ions First Formula First Name First
39 Today s Learning Objectives 1) What is a covalent bond? 2) Compare and contrast a molecule and a compound. 3) What is the difference between polar & nonpolar? 4) Be able to name covalent compounds.
40 Covalent Bonds & Compounds (18-5) The ionic bonds we ve been discussing only work between metals & nonmetals What if two nonmetals come into contact, can they bond with each other?
41 Covalent Bonds & Compounds Covalent Bonds Force of attraction between atoms that result from sharing electrons Between two or more nonmetals
42 Covalent Bonds & Compounds Molecule Neutral group of atoms held together by covalent bonds Ex. H 2 O Molecules are the smallest particle into which a covalently bonded substance can be divided and remain that substance Link 1, Link 2 (start at 50 s)
43 molecules Range from diatomic to very complex
44 Covalent Bonds & Compounds Single and multiple bonds If only 1 pair of electrons is shared, it is a single bond. Ex. H 2 If multiple pairs of electrons are shared, it is a multiple bond. Ex. O 2 and N 2
45 Covalent Bonds & Compounds Two types of covalent bonds Nonpolar bond a covalent bond in which electrons are shared equally between atoms Ex. H 2 Polar bond a covalent bond in which electrons are shared unequally Ex. HCl
46 Covalent Bonds & Compounds Nonpolar & polar bonding result in two types of molecules Nonpolar molecule a molecule that does NOT have oppositely charged ends This type of molecule is symmetrical May have polar or nonpolar bonds Ex. CO 2
47 Covalent Bonds & Compounds Polar molecule unequal sharing of electrons within a molecule, and nonsymmetrical shape, result in oppositely charged ends of the molecule Ex. H 2 O Spoon Activity Simulation (look at polar/nonpolar, & model differences)
48 Covalent Formulas & Names (18-6) We ve named: Monoatomic ions Polyatomic ions Binary ionic compounds Now: Binary molecular compounds
49 Covalent Formulas & Names Naming Binary Molecular Compounds When 2 non-metals combine, usually get Binary Molecular Compound Name is 2 words First word is name of the element listed first. A Greek prefix is used to show the number of atoms present (only if >1) Know all 10 Greek prefixes
50 Covalent Formulas & Names Greek prefixes: 1 = mono- 2 = di- 3 = tri- 4 = tetra- 5 = penta- 6 = hexa- 7 = hepta- 8 = octa- 9 = nona- 10 = deca-
51 Covalent Formulas & Names Second word consists of: The appropriate Greek prefix showing the number of atoms of that element The stem name of the 2nd element The suffix -ide Ex. N 2 O 4 is dinitrogen tetroxide Game
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