activity 1-5. draw a picture of the spectrum draw the four lines in the hydrogen spectrum under the...
TRANSCRIPT
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Activity 1-5
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Activity 1-5
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• Draw a picture of the spectrum• Draw the four lines in the hydrogen
spectrum under the whole spectrum• Label the four lines:
Red 656 nm
Green 486 nm
Blue 434 nm
Violet 410 nm
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Activity 1-6—EC’sValence=last energy level!
1. Which elements have 1 valence e-?
2. Which elements have 3 valence e-?
3. Which elements have 4 valence e-?
4. Which elements have 5 valence e-?
5. Which elements have 6 valence e-?
6. Which elements have 7 valence e-?
7. Which elements have a full valence level?
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Ionization energies
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 360
20
40
60
80
100
120
140
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In your notes:
Define:
X + 1st I.E. X+ + 1e-
X+ + 2nd I.E. X+2 + 1e-
For example
Mg + 1st I.E. Mg+ + 1e-
As+ + 2nd I.E. As+2 + 1e-
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In your notes:1) How does the 1st ionization energy
change as you go across a row? (period.)
2) How does the 1st ionization energy change as you go down a column? (group)
3) How do these changes relate to the size of the atoms?
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In your notes:4) Where does the 1st ionization energy
graph have peaks?
5) Where does the 1st ionization energy graph fall?
6) Where does the 2nd ionization energy graph have peaks?
7) Where does the 2nd ionization energy graph fall?
8) How does the ionization energy relate to electron configuration?
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In your notes:9) Compare the 1st ionization energies of
metals in a row to the non-metals in the same row.
10)Compare the sizes of the metal atoms in a row to the sizes of the non-metals in the same row.
11)Compare the electron configurations of the metals in a row to the non-metals in the same row.
12) What makes an element a metal?
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On your graph:
• Make a note of the answers to questions 1-12 on the graph.
• Include an arrow from each answer to a part of the graph that relates to the answer.
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Activity 1-7
• How and why does an atom ionize?
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Valence energy
level EC
# e- invalence
level
Total electron
#
Noble gasses
HeliumNeonArgonXenonRadon
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Loses ___ e-
# e- more than last
noble gas
EC(valence
level)
Ion charge
Metals
NaK
CaMgSrAl
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Gains ___ e-
# e- less than nextnoble gas
EC(valence
level)
Ion charge
Nonmetals
NOFSClBr
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Why does the oxide ion have 10 e-?
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Why does the oxide ion have 10 e-?
• (Does your answer include:
How many e- does an oxygen atom have?
What is its EC?
Does it gain or lose e-? Metal or Nonmetal?
How many? What is the charge on the ion?
What EC does it attain?
…and “Everybody wants to be a noble gas!”
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Why does the strontium ion have 36 e-?
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Why does the strontium ion have 36 e-?
• (Does your answer include:
How many e- does an strontium atom have?
What is its EC? Metal or nonmetal?
Does it gain or lose e-?
How many? Charge on ion?
What EC does it attain?
…and “Everybody wants to be a noble gas!”
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How many electrons does a beryllium ion have? Why?
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Name an ion that has 54 e-. Why does it have this many?
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Activity 1-8
• Forming ionic compounds.
• An electron dot diagram shows a symbol with one dot for each valence electron.
Al Br
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Make a poster to show the formation of an ionic compound
1) Choose a metal and a nonmetal
2) Draw electron dot diagrams for each
3) Draw arrows to show the transfer of electrons
4) Add atoms to provide or accept enough electrons to empty and fill valence levels
5) Draw the ions after the transfer, with valence electrons and charges
6) Write the reaction
7) Name the product
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Nomeclature
One name for each substance, one substance for each (valid)
name
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Formulas
• A formula shows the number and type of atoms in a compound
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Formulas
• A formula shows the number and type of atoms in a compound
Na2SO3
……means…
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Formulas
• A formula shows the number and type of atoms in a compound
Na2SO3
Two sodium
One sulfur
Three oxygen
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Formulas
• A formula shows the number and type of atoms in a compound
Fe2(CrO4)3
……means…
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Formulas
• A formula shows the number and type of atoms in a compound
Fe2(CrO4)3
……means…
(distribute the “3”)
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Formulas
• A formula shows the number and type of atoms in a compound
Fe2(CrO4)3
Two iron Three chromium
Twelve oxygen
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If it is a…
• The nomenclature rules depend on what type of substance. They include:
1. Ionic compounds
2. Covalent compounds
3. Acids
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If it is a…
• The type of substance refers to it’s elements:
1. Ionic compounds—begins with a metal
2. Covalent compounds—no metals
3. Acids—begins with H
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO• BaCl2• Na2SO3
• NiBr3
• Fe2(CrO4)3
Name the ions
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO magnesium oxide• BaCl2• Na2SO3
• NiBr3
• Fe2(CrO4)3
Name the ions
Not “oxygen”
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO magnesium oxide• BaCl2 barium chloride
• Na2SO3
• NiBr3
• Fe2(CrO4)3
Name the ions
Not “dichloride”
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO magnesium oxide• BaCl2 barium chloride
• Na2SO3 sodium sulfite
• NiBr3
• Fe2(CrO4)3
Name the ions
Look it up!
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Now, wait a minute
• Two compounds of bromine and nickel:
NiBr3 and NiBr2
• Not both nickel bromide
Transition element ions are written with a Roman numeral to show the charge.
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO magnesium oxide• BaCl2 barium chloride
• Na2SO3 sodium sulfite
• NiBr3 nickel (III) bromide
• Fe2(CrO4)3
Name the ions
+ charge on the metal
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• MgO magnesium oxide• BaCl2 barium chloride
• Na2SO3 sodium sulfite
• NiBr3 nickel (III) bromide
• Fe2(CrO4)3 iron (III) chromate
Name the ions
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• NaBr• K2O
• (NH4)2CO3
• FeS• CrI3
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Ionic compounds: Formula to name
• Name (don’t count) the ions.
• NaBr sodium bromide• K2O potassium oxide
• (NH4)2CO3 ammonium carbonate
• FeS iron (II) sulfide• CrI3 chromium (III) iodide
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Warnings
• Groups 1, 2 and aluminum do NOT get a Roman numeral
• Count your charges to get the transition element charge.
• Roman numeral is part of an ion’s name
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Ionic compounds: Name to formula
• Balance your charges
• Lithium chloride • calcium bromide • Aluminum sulfate• cobalt (II) oxide • nickel (III) nitrite
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Ionic compounds: Name to formula
• Balance your charges
• Lithium chloride LiCl• calcium bromide CaBr2
• Aluminum sulfate Al2(SO4)3
• cobalt (II) oxide CoO• nickel (III) nitrite Ni(NO2)3
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Warnings
• Use () when you double or triple a polyatomic ion
• Balance your charges
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Prefixes (Back of your chart)
1. Mono-
2. Di-
3. Tri-
4. Tetra-
5. Penta-
6. Hexa-
7. Hepta-
8. Octo-
9. Nona-
10. Deca-
11. Undeca-
12. Dodeca-
13. Trisdeca-
…
20. Icosa-
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Covalent compounds: Formula to name
• Name the atoms, in order, with prefixes (ends in –ide)
• N2S5
• CCl4• P2O5
• BF3
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Covalent compounds: Formula to name
• Name the atoms, in order, with prefixes (ends in –ide)
• N2S5 dinitrogen pentasulfide
• CCl4 carbon tetrachloride
• P2O5 diphosphorus pentoxide
• BF3 boron trifluoride
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Warnings
• First element is named, second one ends in “–ide”
• “a” or “o” is dropped from prefix before “–oxide”
• “mono-” prefix is omitted on the first atom
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Covalent compounds: Name to formula
• Write the atoms, prefixes become subscripts
• nitrogen trichloride • Arsenic trioxide• Bromine monochloride• Xenon tetrafluoride
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Covalent compounds: Name to formula
• Write the atoms, prefixes become subscripts
• nitrogen trichloride NCl3• Arsenic trioxide AsO3
• Bromine monochloride BrCl• Xenon tetrafluoride XeF4
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Acids
• If the anion name then the acid name• ends in…. is…
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Acids
• If the anion name then the acid name• ends in…. is…• --ide Hydro___ic acid• --ite ___ous acid• --ate ___ic acid
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AcidsFormula to name• HI is _________acid
• HBrO4 is _________acid
• H2CO3 is _________acid
• H2SO3 is ________acid
• HClO is ___________acid
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AcidsFormula to name• HI is hydroiodic acid
• HBrO4 is perbromic acid
• H2CO3 is carbonic acid
• H2SO3 is sulfurous acid
• HClO is hypochlorous acid
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Acids Name to formula
• ____is hydrocyanic acid•
____ is periodic acid
• _____ is phosphoric acid
• _____ is nitrous acid
• ____ is hypoiodous acid
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Acids Name to formula
• HCN is hydrocyanic acid• HIO4 is periodic acid
• H3PO4 is phosphoric acid
• HNO2 is nitrous acid
• HIO is hypoiodous acid
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What is the name?
• K2S
• CrO3
• CaSO4
• Pb(C2H3O2)2
• CuI2
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What is the name?
• K2S Potassium sulfide
• CrO3 Chromium (VI) oxide
• CaSO4 Calcium sulfate
• Pb(C2H3O2)2 Lead (II) acetate
• CuI2 Copper (II) iodide
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• Gold (I) chloride • Lithium oxide • Iron (II) cyanide • Potassium chlorate • Nickel (II) nitrate
What is the formula?
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• Gold (I) chloride AuCl• Lithium oxide Li2O
• Iron (II) cyanide Fe(CN)2
• Potassium chlorate KClO3
• Nickel (II) nitrate Ni(NO3)2
What is the formula?
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• N2O3
• P4O6
• Cl2O
• XeF2
• BrF5
What is the name?
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• N2O3 dinitrogen trioxide
• P4O6 tetraphosphorus hexoxide
• Cl2O dichlorine monoxide
• XeF2 xenon difluoride
• BrF5 bromine pentafluoride
What is the name?
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• Phosphorus trihydride• Dinitrogen monoxide • Bromine monochloride• Xenon trioxide • Iodine heptafluoride
What is the formula?
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• Phosphorus trihydride PH3
• Dinitrogen monoxide N2O
• Bromine monochloride BrCl• Xenon trioxide XeO3
• Iodine heptafluoride IF7
What is the formula?
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• H3PO4
• H2SO3
• HClO3
• H2CrO4
• HCN
What is the name?
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• H3PO4 phosphoric acid
• H2SO3 sulfurous acid
• HClO3 chloric acid
• H2CrO4 chromic acid
• HCN hydrocyanic acid
What is the name?
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• Hypochlorous acid • Hydrobromic acid• Oxalic acid• Nitrous acid• Perchloric acid
What is the formula?
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• Hypochlorous acid HClO• Hydrobromic acid HBr• Oxalic acid H2C2O4
• Nitrous acid HNO2
• Perchloric acid HClO4
What is the formula?
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It’s a puzzlement
• What is the name?
Cu2S
CuS
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It’s a puzzlement
• What is the name?
Cu2S
CuS
Do you get it?
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It’s a puzzlement
• What is the name?
Cu2S
CuS
Copper (I) sulfide
Copper (II) sulfide
Do you get it?
![Page 73: Activity 1-5. Draw a picture of the spectrum Draw the four lines in the hydrogen spectrum under the whole spectrum Label the four lines: Red656 nm Green486](https://reader036.vdocument.in/reader036/viewer/2022062515/56649cd65503460f9499e54d/html5/thumbnails/73.jpg)
It’s a puzzlement
• What is the name?
Cu2S
CuS
Copper (I) sulfide
Copper (II) sulfide
Do you get it?
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• Oxygen gas • Calcium metal• Solid phosphorus• Fluorine gas• Argon gas
What is the formula?
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• Oxygen gas O2
• Calcium metal Ca(s)• Solid phosphorus P4
• Fluorine gas F2
• Argon gas Ar
What is the formula?
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• Mn(s) • H2
• I2
• S8
• Br2
What is the name?
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• Mn(s) manganese metal• H2 hydrogen gas
• I2 solid iodine
• S8 solid sulfur
• Br2 liquid bromine
What is the name?
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Name these compounds
• Common Name Chemical Formula• a. Sugar of lead Pb(C2H3O2) 2
• b. Blue vitrol CuSO4
• c. Epsom salts MgSO4•7H2O
• d. Milk of magnesia Mg(OH) 2
• e. Gypsum CaSO4
• f. Laughing gas N2O
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Write the formula
• Sulfur difluoride • Sulfur hexafluoride • Sodium dihydrogen phosphate • Lithium nitride • Chromium (III) carbonate • Tin (II) fluoride
• Ammonium acetate • Ammonium hydrogen sulfate • Cobalt (III) nitrate • Mercury (I) chloride • Potassium chlorate • Sodium hydride
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What is the name?
NaCl RbBr CsF
AlI3 HI NO
NF3 N2F4 N2Cl2 SiF4
H2Se HNO3 HNO2
H3PO4 H3PO3 NaHSO4 Ca(HSO3)2 Ru(NO3)3 V2O5