* Determine how many moles are in 435 grams of NaCl. Significant figures matter so make sure you have the correct amount.

Mr. Berlin Luskin Academy

* Objective: I will be able to identify the difference between ionic and covalent bonds and determine which atoms will form these bonds. LecturePLUS Timberlake 99

* Molecule: Two or more atoms bonded together to form a compound. * Ionic bond: when atoms are attracted to each other due to ionic states of the atom. * Covalent bond: when a bond is formed by sharing of electrons between atoms. * Single Bond: Shares one pair of electrons in a covalent bond. * Double Bond: Shares two pairs of electrons in a covalent bond. * Triple Bond: Shares three pairs of electrons in a covalent bond. * Mole: The measurement of grams in a formula or atom. (same as atomic mass. Also, 1 mole = x atoms). * Chemical Formula: The correct expression for the number of atoms in a compound. LecturePLUS Timberlake 99

Attraction between + ions (cations) and – ions (anions) Electrons go from metals to nonmetals electron transfer metal nonmetal ion + ion – Electrons lost = Electrons gain

Formulas of ionic compounds are determined from the charges on the ions atoms ions     – Na  +  F :  Na + : F :  NaF     sodium fluorine sodium fluoride formula Charge balance: = 0

Write the formula for the ionic compound that will form between Ba 2+ and Cl . Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl  Cl  3. Write the number of ions needed as subscripts BaCl 2

Contain 2 different elements Name the metal first, then the nonmetal as - ide. Use name of a metal with a fixed charge Groups 1, 2, 3 and Ag, Zn, and Cd Examples: NaClsodium chloride ZnI 2 zinc iodide Al 2 O 3 aluminum oxide

Complete the names of the following binary compounds: Na 3 Nsodium nitride KBrpotassium bromide Al 2 O 3 aluminum oxide MgSmagnesium sulfide

Many form 2 or more positive ions or or 3+ Ag + Cd 2+ Cu +, Cu 2+ Fe 2+, Fe 3+ silver cadmium copper(I) ion iron(II) ion ion ion copper (II) ion iron(III) ion Zn 2+ zinc ion

Use a roman number after the name of a metal that forms two or more ions Transition metals and the metals in groups 4A and 5A FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ )lead (II) chloride Fe 2 S 3 (Fe 3+ )iron (III) sulfide

Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron (_____) bromide Cu 2 Ocopper (_____) oxide SnCl 4 ___( IV ) ________________ Fe 2 O 3 ________________________ CuS________________________

Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron ( II ) bromide Cu 2 Ocopper ( I ) oxide SnCl 4 tin (IV) chloride Fe 2 O 3 iron (III) oxide CuScopper (II) sulfide

LecturePLUS Timberlake 14 Formed between two nonmetals in 4, 5, 6, and 7 Nonmetals have high electronegativity values Electrons are shared single bond shares one pair electrons double bond shares two pairs electrons triple bond shares three pairs electrons

LecturePLUS Timberlake 15 Indicate whether a bond between the following would be 1) Ionic2) covalent ____A. sodium and oxygen ____B. nitrogen and oxygen ____C. phosphorus and chlorine ____D. calcium and sulfur ____E. chlorine and bromine

LecturePLUS Timberlake 16 Indicate whether a bond between the following would be 1) Ionic2) covalent 1A. sodium and oxygen 2B. nitrogen and oxygen 2C. phosphorus and chlorine 1D. calcium and sulfur 2E. chlorine and bromine

* Share electrons * Held together by actual sharing of the electrons * Low boiling/melting points * Do not dissolve in water * Not brittle * Not conductive * Loss or gain electrons * Held together by +/- forces. * High boiling/melting points * Dissolve in water * Brittle compounds * Salts * conductive

LecturePLUS Timberlake 18 Gases that exist as diatomic molecules are H 2, F 2, N 2, O 2, Cl 2, Br 2, and I 2. These molecules just keep their original names. octets          N  +  N   N ::: NTriple bond  Example: O 2 is just oxygen

LecturePLUS Timberlake 19 Use the name of the element to name the following diatomic molecules. H 2 hydrogen N 2 nitrogen Cl 2 _______________ O 2 _______________ I 2 _______________

LecturePLUS Timberlake 20 Use the name of the element to name the following diatomic molecules. H 2 hydrogen N 2 nitrogen Cl 2 chlorine O 2 oxygen I 2 iodine

LecturePLUS Timberlake 21 Two nonmetals Name each element End the last element in -ide Add prefixes to show more than 1 atom Prefixes mon1 penta5 di2hexa6 tri3hepta7 tetra4octa8

LecturePLUS Timberlake 22 Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon _______________ PCl 3 phosphorus _______chloride CCl 4 carbon ________chloride N 2 O_____nitrogen _____oxide

LecturePLUS Timberlake 23 CO carbon monoxide CO 2 carbon dioxide PCl 3 phosphorus trichloride CCl 4 carbon tetrachloride N 2 Odinitrogen monoxide

LecturePLUS Timberlake 24 The attraction of an atom for electrons is called its electronegativity. Fluorine has the greatest electronegativity. The metals have low electronegativities.

LecturePLUS Timberlake 25 Nonpolar covalent bond Electrons are shared between atoms with the same electronegativity values. Difference = 0 Examples: N 2 Br 2 O 2

LecturePLUS Timberlake 26 A.P 2 O 5 3) diphosphorus pentoxide B.Cl 2 O 7 1) dichlorine heptoxide C. Cl 2 1) chlorine

LecturePLUS Timberlake 27 Nonpolar covalent bond Electrons are shared between atoms with the same electronegativity values. Difference = 0 Examples: N 2 Br 2 O 2

LecturePLUS Timberlake 28 Polar covalent bond Electrons are shared between different nonmetal atoms Examples: O-Cl O-SN-ClH 2 O

LecturePLUS Timberlake 29 Identify the type of bond between the following atoms A. K-N 1) nonpolar2) polar3) ionic B. N-O 1) nonpolar2) polar3) ionic C. Cl-Cl 1) nonpolar2) polar3) ionic

LecturePLUS Timberlake 30 A. K-N3) ionic B. N-O2) polar C. Cl-Cl 1) nonpolar

LecturePLUS Timberlake 31 Match each set with the correct name: A. Na 2 CO 3 1) magnesium sulfite MgSO 3 2) magnesium sulfate MgSO 4 3) sodium carbonate B.Ca(HCO 3 ) 2 1) calcium carbonate CaCO 3 2) calcium phosphate Ca 3 (PO 4 ) 2 3) calcium bicarbonate

LecturePLUS Timberlake 32 A. Na 2 CO 3 3) sodium carbonate MgSO 3 1) magnesium sulfite MgSO 4 2) magnesium sulfate B.Ca(HCO 3 ) 2 3) calcium bicarbonate CaCO 3 1) calcium carbonate Ca 3 (PO 4 ) 2 2) calcium phosphate

LecturePLUS Timberlake 99 Chemical reactions are classified into four general types Combination Decomposition Single Replacement Double Replacement

LecturePLUS Timberlake 99 Two or more elements or simple compounds combine to form (synthesize) one product A + B AB 2Mg + O 2 2MgO 2Na + Cl 2 2NaCl SO 3 + H 2 OH 2 SO 4

LecturePLUS Timberlake 99 One substance is broken down (split) into two or more simpler substances. ABA + B 2HgO2Hg + O 2 2KClO 3 2KCl + 3 O 2

LecturePLUS Timberlake 99 Classify the following reactions as 1) combination or 2) decomposition: ___A. H 2 + Br 2 2HBr ___B. Al 2 (CO 3 ) 3 Al 2 O 3 + 3CO 2 ___C. 4 Al + 3C Al 4 C 3

LecturePLUS Timberlake 99 Classify the following reactions as 1) combination or 2) decomposition: _1_A. H 2 + Br 2 2HBr _2_B. Al 2 (CO 3 ) 3 Al 2 O 3 + 3CO 2 _1_C. 4 Al + 3C Al 4 C 3

LecturePLUS Timberlake 99 One element takes the place of an element in a reacting compound. A + BC AB + C Zn + 2HCl ZnCl 2 + H 2 Fe + CuSO 4 FeSO 4 +Cu

LecturePLUS Timberlake 99 Two elements in reactants take the place of each other AB + CD AD + CB AgNO 3 + NaCl AgCl + NaNO 3 ZnS + 2HCl ZnCl 2 +H 2 S

LecturePLUS Timberlake 99 Classify the following reactions as 1) single replacement 2) double replacement __ A. 2Al + 3H 2 SO 4 Al 2 (SO 4 ) 3 + 3H 2 __B. Na 2 SO 4 + 2AgNO 3 Ag 2 SO 4 + 2NaNO 3 __C. 3C + Fe 2 O 3 2Fe + 3CO

LecturePLUS Timberlake 99 Classify the following reactions as 1) single replacement 2) double replacement 1_ A. 2Al + 3H 2 SO 4 Al 2 (SO 4 ) 3 + 3H 2 2_B. Na 2 SO 4 + 2AgNO 3 Ag 2 SO 4 + 2NaNO 3 1_C. 3C + Fe 2 O 3 2Fe + 3CO

LecturePLUS Timberlake 99 A reaction in which a compound (often carbon) reacts with oxygen C + O 2 CO 2 CH 4 + 2O 2 CO 2 + 2H 2 O C 3 H 8 + 5O 2 3CO 2 + 4H 2 O C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O

LecturePLUS Timberlake 99  Reactions that involve a loss or gain of electrons  Occurs in many of the 4 types of reactions and combustion  Important in food metabolism, batteries, rusting of metals

LecturePLUS Timberlake 99 Electrons are transferred Two processes occur Oxidation = Loss of electrons (LEO) ZnZn e - Reduction = Gain of electrons (GER) Cu e - Cu

LecturePLUS Timberlake 99 In organic and biological reactions oxidation = Loss of H reduction = Gain of H

LecturePLUS Timberlake Fe + 3 O 2 2 Fe 2 O 3 Fe and O 2 4 mole Fe and 3 mole O 2 3 mole O 2 4 mole Fe Fe and Fe 2 O 3 4 mole Feand2 mole Fe 2 O 3 2 mole Fe 2 O 3 4 mole Fe O 2 and Fe 2 O 3 3 mole O 2 and 2 mole Fe 2 O 3 2 mole Fe 2 O 3 3 mole O 2

LecturePLUS Timberlake H 2 (g) + N 2 (g) 2 NH 3 (g) A. A mole factor for H 2 and N 2 is 1) 3 mole N 2 2) 1 mole N 2 3) 1 mole N 2 1 mole H 2 3 mole H 2 2 mole H 2 B. A mole factor for NH 3 and H 2 is 1) 1 mole H 2 2) 2 mole NH 3 3) 3 mole N 2 2 mole NH 3 3 mole H 2 2 mole NH 3

LecturePLUS Timberlake H 2 (g) + N 2 (g) 2 NH 3 (g) A. A mole factor for H 2 and N 2 is 2) 1 mole N 2 3 mole H 2 B. A mole factor for NH 3 and H 2 is 2) 2 mole NH 3 3 mole H 2

LecturePLUS Timberlake Fe + 3 O 2 2 Fe 2 O 3 How many moles of Fe are needed to react with 12.0 mole of O 2 ? 1) 3.00 mole Fe 2) 9.00 mole Fe 3) 16.0 mole Fe

LecturePLUS Timberlake Fe + 3 O 2 2 Fe 2 O mole O 2 x 4 mole Fe = 16.0 mole Fe 3 mole O 2

* Formula mass is the sum of the atomic mass weights of each element in a empirical formula. To calculate, simply add up the average atomic mass of each atom. * Example: * NaClNa =22.99 grams * Cl=35.45 grams * total58.44 grams

* Example: * BeCl 2 Be =9.01 grams * 2 x Cl=70.90 grams * total79.91 grams

LecturePLUS Timberlake The reaction between H 2 and O 2 produces 13.1 g of water. How many grams of O 2 reacted? Write the equation H 2 (g) + O 2 (g)H 2 O (g) Balance the equation 2 H 2 (g) + O 2 (g)2 H 2 O (g)

LecturePLUS Timberlake Read an equation in moles 2. Convert given amount to moles 3. Use mole factor to give desired moles 4. Convert moles to grams grams (given)grams (desired) moles (given)moles (desired)