Bonding (Taylor Williams) Unit 8

Determine the number of each atom in Al(NO3)3.

9 atoms of oxygen, 3 nitrogen atoms, and 1 aluminum atom

Draw an electron dot diagram for the following compounds.

AlBr3

examples

Aluminum and Chlorine AlCl3 Lithium and Nitrogen Li3N Magnesium and Iodine MgI2 Calcium and Oxygen CaO Sodium and Sulfur Na2S

Determine the name for the compound (NH4)2S.

Ammonium sulfide

Name the following covalent compounds:

BBr3 Boron tribromide CF4 Carbon tetrafluoride P2S3 Diphosphorous trisulfide NH3 Nitrogen trihydride

examples

Barium sulfate Ba(SO4) Aluminum carbonate Al2(CO3)3 Calcium nitrate Ca(NO3)2 Sodium acetate NaC2H3O2 Potassium phosphate K3PO4

Determine the name for the compound BBr3.

Boron tribromide

Draw an electron dot diagram for the following compounds

CO2

examples

CO2 Carbon dioxide H2O Dihydrogen monoxide CH4 Carbon tetrahydride PCl3 Phosphorus trichloride P4O10 Tetraphosphorus decaoxide

Draw an electron dot diagram for the following compounds.

Ca3P2

List the number of atoms of each element in the compounds below.

CaCl2- 1 Ca, 2 Cl Na2SO4-2 Na, 1 S, 4 O Al2(SO4)3-2 Al, 3 S, 12 O CCl4-1 C, 4 Cl (bottom numbers)

Determine the name for the compound CaCO3.

Calcium carbonate

Determine the name for the compound CF4.

Carbon Tetrafluoride

Explain the difference between a cation and an anion, including how each are formed and an example of each.

Cation: positively charged ion formed from losing e-, Ex. Ca+2 Anion: negatively charged ion formed from gaining e-, Ex. O-2

examples

Copper (II) sulfide CuS Iron (I) nitride Fe3N Manganese (IV) oxide MnO2 Chromium (VI) sulfide CrS3 Titanium (IV) bromide CrS3

Molecules are compounds formed from ______________ bonds.

Covalent bonds

Explain why a covalent bond forms, how it forms, and what types of elements form them.

Covalent bonds form to make elements more stable. Two nonmetals share electrons.

Differentiate between the properties of covalent compounds and ionic compounds.

Covalent compounds: low melting and boiling points, usually gases or dull or brittle solids, do not conduct electricity in water. Ionic compounds: high melting and boiling points, usually solid crystals, do conduct electricity in water.

Determine the name for the compound B2H4.

Diborane(4)

examples

Dicarbon tetraoxide C2O4 Hydrogen monosulfide HS Pentaphosphorus trinitride P5N3 Sulfur pentoxide SO5 Silicon tetrafluoride SiF4

Determine the chemical formula for the following covalent compounds:

Dinitrogen trioxide- N2O3 Sulfur dioxide - SO2 Dinitrogen monosulfide -N2S Diboron tetrahydride - B2H4

electron dot/ lewis dot diagrams

Draw the electron dot structures of the elements.Transfer electrons (using an arrow) from the metal to the nonmetal.Add elements as needed.Continue transferring until all atoms are stable.Write the chemical formula using subscripts to show how many of each element were needed.

Explain why elements form compounds, and what most elements need to achieve this. Include which elements do not tend to form compounds and why.

Elements form compounds to be stable. Most elements need 8 valence electrons in their outermost energy level to achieve this. Noble gases tend to not form compounds because they already have full outer energy levels of electrons.

Compounds with high melting points are usually ___________.

Ionic

Explain why an ionic bond forms, how it forms, the two parts that make it up, and the overall charge of the resulting compound.

Ionic bonds form to make elements more stable. A metal (cation) transfers its valence e- to a nonmetal (anion). Overall charge is 0.

Determine the name for the compound Fe(NO3)2.

Iron(II) nitrate

Draw an electron dot diagram for the following compounds.

KI

Determine the chemical formula for the following ionic compounds:

Lithium phosphate Li3PO4 Silver (I) chloride AgCl Calcium chlorate Ca(ClO3)2 Iron (III) bromide FeBr3 Magnesium hydroxide Mg(OH)2 Ammonium acetate NH4C2H3O2 (bottom numbers)

examples

MgCl2 Magnesium chloride (NH4)3PO4 Ammonium phosphate Ni(OH)2 Nickel (II) hydroxide

Draw an electron dot diagram for the following compounds:

N2

examples

Na3PO4 Sodium phosphate MgSO4 Magnesium sulfate NH4Cl Ammonium chloride with exception 1 NaNO3 Sodium Nitrate CaSO4 Calcium Sulfate (NH4)2O Ammonium Oxide Mg3(PO4)2 Magnesium Phosphate NH4NO3 Ammonium Nitrate

Name the following ionic compounds:

NaC2H3O2 Sodium acetate Mg(OH)2 Magnesium hydroxide Al2O3 Aluminum oxide MnOH Manganese (I) hydroxide (NH4)2SO4 Ammonium sulfate AuCO3 Gold (II) carbonate

how to determine the name for a covalent copound- formula to name

Name first element with prefix to indicate how many. Exception: don't use mono for "1" for 1st elementName second element with prefix to indicate how many AND add an -ide ending.

steps for naming ionic compounds- formula to name

Name the metal (cation) Exception #1 = If polyatomic ion, use its special name Exception #2 = If a transition metal, use a Roman Numeral to indicate the charge of the metal Name the nonmetal (anion) with -ide ending Exception #1 = If polyatomic ion, use its special name, no -ide

Classify the following as atoms, ionic compounds, or molecules:

Ne- Atom KCl- Ionic compound H2O- Ionic compound NH4Cl- Molecule

Why does Neon rarely form compounds?

Noble Gases have a full valence shell, which is why they rarely form bonds with other atoms.

determining the roman numeral

Option 1: Reverse criss cross Option 2: Use visuals or math to determine what charge of cation must be for overall charge to be zero. ex. CuCl Copper (I) Chloride CuCl2 Copper (II) Chloride

Determine the chemical formula for phosphorous pentabromide.

PBr5

Draw an electron dot diagram for the following compounds

PCl3

Determine the name for the compound PBr3.

Phosphorus tribromide

Determine the name for the compound KOH.

Potassium hydroxide

Describe the difference between single, double, and triple bonds.

Single bond: 2 e- shared Double bond: 4 e- shared Triple bond: 6 e- shared

Determine the name for the compound NaC2H3O2.

Sodium acetate

examples

Sodium chloride NaCl Aluminum hydroxide Al(OH)3 Iron (III) oxide Fe2O3

how to determine the formula for a covalent compound - name to formula

Use prefixes to determine subscripts. NO CRISS CROSSES OR SIMPLIFYING IN COVALENT!!!

hints

When determining the Roman numeral for a transitional metal, try to reverse crisscross first. If the subscript doesn't match the charge of the known nonmetal, then it must have been simplified. When it doesn't match, do a little trial and error. Double check your work by going the opposite way (determining formula from name) and see if your results match what you started with. Always put parentheses around polyatomic ions so you remember to "protect" them. You CANNOT change the subscripts of the polyatomic ions, so using parentheses will help you to remember that!

how to determine the chemical formula for an ionic compound- name to formula

Write down the ions of each element with charge. (aka the symbol with its oxidation #)Determine the # of each ion it takes to make a compound with no charge. (aka "crisscross applesauce" the charges)Write down the formula using subscripts to show how many of each ion it took.Reduce/simplify. (if needed)

steps for writing chemical formulas for ionic compounds - name to formula

Write down the ions with charge Crisscross the charges to determine subscripts (aka "criss cross applesauce") (keep subscripts outside of parentheses and don't change ANYTHING inside) Rewrite with subscripts Reduce/simplify (if needed)

how to name ionic compounds- formula to name

Write the name of the first element. (the metal)Write the name of the second element (the nonmetal) with an -ide ending.

Would elements ever not benefit from forming compounds?

YES if they are already stable 🡪 which the noble gases are!

Determine the name for the compound ZnSO4.

Zinc sulfate

poly atomic ions

a positively or negatively charged, covalently, bonded group of atoms

octect rule

atoms will gain, lose, or share electrons in order to have 8 electrons in their outer shell

covalent bond

bond that results from the sharing of electrons between two nonmetals

ions

charged atom that has gained or lost electrons

molecule

compound formed when 2 or more elements bond covalently.

chemical bond

force that holds atoms together in a compound There are many types of bonds that can form, and not all bonds are created equal. We will start by looking at ionic bonds.

Stability

full/complete outer energy level of valence electrons

exceptions

if polyatomic ion, use special name if polyatomic ion, use special name. No -ide ending.

two main types of bonds

ionic and covelent

anions

negatively charged ions; atoms or molecules that have gained e- Usually nonmetals

chemical formula

tells what elements and how many of each element are in a unit of that compound Examples:H2O - water; contains 2 atoms of hydrogen and 1 atom of oxygen NH3 - ammonia; contains 1 atom of nitrogen and 3 atoms of hydrogen

Oxidation numbers

the charge of an ion within a compound Written as a superscript to the right of the symbol Group 1 elements have 1 valence e- 🡪 +1 charge Group 2 elements have 2 valence e- 🡪 +2 charge Skip groups 3-12 transition metals Group 13 elements have 3 valence e- 🡪 +3 charge Group 14 elements have 4 valence e- 🡪 +/- 4 charge Group 15 elements have 5 valence e- 🡪 -3 charge Group 16 elements have 6 valence e- 🡪 -2 charge Group 17 elements have 7 valence e- 🡪 -1 charge

oxidation numbers

the charge on an ion Written as a superscript to the right of the symbol Group 1 elements have 1 valence e- 🡪 +1 charge Group 2 elements have 2 valence e- 🡪 +2 charge

compound

two or more elements chemically combined the properties of a compound are very different from the properties of the elements that make up the compound Ex. Na and Cl are very different from NaCl

iconic bond

when atoms transfer electrons in order to be stable Usually between a metal and a nonmetal Results in the formation of ions

how to determine the formula for an ionic compound with polyatomic ions- name to formula

write down the ions of each element with charge ( aka the symbol with its oxidation number ) determine the number of each ion it takes to make a compound with no charge( crisscross) (with no charge) (aka "criss cross applesauce" the charges) (keep subscripts outside of parentheses and don't change ANYTHING inside) write down the formula using subscripts to show how many of each ion it took

how to determine the formula for an ionic compound with transition metals - name to formula

write down the ions of each element with charge( symbol with oxidation number) determine the number of each ion it takes to make a compound with no charge(crisscross)with no charge write down the formula using subscripts (bottom) to show how many of each ion it took reduce if needed

how to name ionic compounds with transition metals- formula to name

write the name of the first element the metal (if a transition metal, include a Roman numeral to indicate the charge of the metal) write the name of the second element the nonmetal with an ide ending