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