3. Have your Bonding Paper out from yesterday. HOMEWORK TOO! 1. Complete Covalent Bond Diagrams. 2. Compare/Contrast Bonds 3. Notes 4.
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1 April 18, 2012 Honors 1. Pick up your paper. 2. Have a seat quietly! 3. Have your Bonding Paper out from yesterday. HOMEWORK TOO! Agenda 1. Complete Covalent Bond Diagrams. 2. Compare/Contrast Bonds 3. Notes 4. ION Homework Ion, Periodic Table Quiz tomorrow! electronegativity, ion, valence, oxidation number, covalent bond, ionic bond, octet rule
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4 1 How many valance electrons does Sodium have? How many valence electrons does Chlorine have? 2 How many electrons does Chlorine need to complete its outer shell? 3 How many electrons does Sodium need to lose to be left with a complete shell? 4 Since Sodium lost one electron, what is its charge? What do we call a positively charged ion? 5 Since Chlorine gained one electron, what is its charge? What do we call a negatively charged ion? 6 Do the charges balance? 7 - What is the chemical formula for this compound? 8 What is the name of this compound?
5 Apr 19 10:19 AM homework
6 homework Apr 19 10:24 AM homework Apr 19 10:29 AM
7 1 How many valance electrons does Hydrogen have? 2 How many valance electrons does Chlorine have? 3 How many electrons does each atom need to have a complete shell? 4 - How many electrons does the Hydrogen atom now have? How many does the Chlorine atom have? 5 - What is the chemical formula for this compound?
8 Negative Ions Br N H Na Ca O Cl Mg Place all the negative ions in this box H Cl Click this box to check your answers N Br O Negative ions
9 1 Positive Ions Br O H Na Ca N Cl Mg Place all the positive ions in this box Click this box Mg to check your answers Ca Na positive ions Rules to REMEMBER 1. Oxidation numbers are the back bone to writing the correct formula for compounds 2. Make sure you use the correct charge with each element to be able to complete the formula EXAMPLE: Write the correct formula with the following 2 elements: Ca & Cl Ca +2 1 Cl Since the charges are different you will need to use subscripts to indicate the ratio of ions in the formula Ca +2 Cl 1 Ca 1 Cl +2 Step 1: Cross the charges over Ca1 Cl 2 CaCl 2 Step 2: Drop the charges Step 3: Write the completed formula
10 Practice Problems 1. K & S 2. Mg & O 3. Na & F *the subscripts cancel each other out *the subscripts cancel each other out Practice Problems 1. K & S K +1 S 2 K 2 S 2. Mg & O Mg +2 O 2 MgO *the subscripts cancel each other out 3. Na & F Na +1 F 1 NaF *the subscripts cancel each other out
11 1 What is the correct formula for Barium and Phosphorus 2 What is the correct formula for Magnesium and Bromine
12 Ionic bonds Covalent bonds Take and give electrons Share electrons Positive and negative ions negative and negative ions ionic and covalent bonding Steps for determining ionic and covalent bonds Figure out valence electrons Will the atom steal or give? 1, 2 or 3 will give and 5, 6, or 7 will steal If it gives it will become a positive ion. It will be positive the number it needs to get rid of. If it steals it will become a negative ion. It will be negative the number it needs to steal to get 8. Negative & negative will be covalent, negative & positive will be ionic. Steps ionic/covalent
13 Why do atoms combine? Compounds-- 2 or more elements joined in a certain ratio showing properties different from the elements from which it is made Elements are attached to each other in a certain ratio. Form in a chemical change involving energy and electrons. Bonding of atoms achieves chemical stability. Elements lose gain or share electrons to become stable because... 8IS GREAT! Metals Have luster, are malleable and ductile, good conductors of heat and electricity Lose electrons to nonmetal atoms to form positively charged ions in ionic bonds Large atomic radii compared to nonmetal atoms Low electronegativity and ionization energy Left side of the periodic table (except H)
14 Nonmetals Are dull and brittle, poor conductors Gain electrons from metal atoms to form negatively charged ions in ionic bonds Share unpaired valence electrons with other nonmetal atoms to form covalent bonds and molecules Small atomic radii compared to metal atoms High electronegativity and ionization energy Right side of the periodic table (except Group 18) Metalloids Found lying on the jagged line between metals and nonmetals flatly touching the line (except Al and Po). Share properties of metals and nonmetals (Si is shiny like a metal, brittle like a nonmetal and is a semiconductor).
15 Diatomic Molecules Br, I, N, Cl, H, O and F are so reactive that they exist in a more chemically stable state when they covalently bond with another atom of their own element to make two-atom, or diatomic molecules. Br2, I2, N2, Cl2, H2, O2 and F2 The decomposition of water: 2 H2O or 2 H2 + O2 Electronegativity An atom s attraction to electrons in a chemical bond. F has the highest, at 4.0 Fr has the lowest, at 0.7 If two atoms that are different in EN (END) from each other by 1.7 or more collide and bond (like a metal atom and a nonmetal atom), the one with the higher electronegativity will pull the valence electrons away from the atom with the lower electronegativity to form a (-) ion. The atom that was stripped of its valence electrons forms a (+) ion. If the two atoms have an END of less than 1.7, they will share their unpaired valence electrons covalent bond!
16 Ionization Energy The energy required to remove the most loosely held valence electron from an atom in the gas phase. High electronegativity means high ionization energy because if an atom is more attracted to electrons, it will take more energy to remove those electrons. Metals have low ionization energy. They lose electrons easily to form (+) charged ions. Nonmetals have high ionization energy but high electronegativity. They gain electrons easily to form (-) charged ions when reacted with metals, or share unpaired valence electrons with other nonmetal atoms. Ions Ions are charged particles formed by the gain or loss of electrons. Metals lose electrons (oxidation) to form (+) charged cations. Nonmetals gain electrons (reduction) to form (-) charged anions. Atoms will gain or lose electrons in such a way that they end up with 8 valence electrons (stable octet). The exceptions to this are H, Li, Be and B, which are not large enough to support 8 valence electrons. They must be satisfied with 2 (Li, Be, B) or 0 (H).
17 ION worksheet Homework Ion, Periodic Table, Bonding Quiz tomorrow!
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Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck atoms- the smallest particle of an element that can be identified with that element are the building blocks of matter consists of protons and
We will not be doing these type of calculations however, if interested then can read on your own
Chemical Bond Lattice Energies and Types of Ions Na (s) + 1/2Cl 2 (g) NaCl (s) ΔH= -411 kj/mol Energetically favored: lower energy Like a car rolling down a hill We will not be doing these type of calculations
Candidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
3/5/2014. iclicker Participation Question: A. MgS < AlP < NaCl B. MgS < NaCl < AlP C. NaCl < AlP < MgS D. NaCl < MgS < AlP
Today: Ionic Bonding vs. Covalent Bonding Strengths of Covalent Bonds: Bond Energy Diagrams Bond Polarities: Nonpolar Covalent vs. Polar Covalent vs. Ionic Electronegativity Differences Dipole Moments