Atomic Theory Practice

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Atomic Theory Practice Atomic Theory Practice Name the element: 1. Na 23 11 2. ? 32 16 3. ? 14 6 4. ? 39 19 + 5. Group IIA, Period 3 6. 1s 2 2s 2 2p 5 Sodium Sodium Sulfur Sulfur Carbon-14 Carbon-14 Potassium Potassium ion ion Magnesium Magnesium Fluorin Fluorin e e

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Atomic Theory Practice. Name the element: Na 23 11 ? 32 16 ? 14 6 ? 39 19 + Group IIA, Period 3 1s 2 2s 2 2p 5. Sodium. Sulfur. Carbon-14. Potassium ion. Magnesium. Fluorine. MOLECULAR MADNESS. Bonding, Shape, Polarity & Reactions. ATOMIC THEORY. - PowerPoint PPT Presentation

Transcript of Atomic Theory Practice

Page 1: Atomic Theory Practice

Atomic Theory PracticeAtomic Theory Practice

Name the element:

1. Na2311

2. ?3216

3. ?146

4. ?3919

+

5. Group IIA, Period 3

6. 1s22s22p5

SodiumSodium

SulfurSulfur

Carbon-14Carbon-14

Potassium ionPotassium ion

MagnesiumMagnesium

FluorineFluorine

Page 2: Atomic Theory Practice

MOLECULAR MOLECULAR MADNESSMADNESSBonding, Shape, Polarity & Bonding, Shape, Polarity &

ReactionsReactions

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ATOMIC THEORYATOMIC THEORY

ProtonsProtons NeutronsNeutrons ElectronsElectrons

+ 0 -

Nucleus Nucleus Orbitals

Atomic # Atomic mass – atomic #

Atomic #

Unchangeable IsotopesIsotopes IonsIons• CationCation +

•Less e-• AnionAnion –

•More e-

• Atoms composed of subatomic particles

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Exothermic Exothermic (heat emitting, i.e. chem warm up :) (heat emitting, i.e. chem warm up :)

Exercise #1Exercise #1

A. Draw the Lewis structure for Carbon.

B. Why do atoms bond with one another?

C. What are the 2 main types of intramolecular bonds?

To fill their valence shell (Octet Rule)

1.1. IonicIonic – transfer electrons2.2. CovalentCovalent – share electrons

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BONDINGBONDINGIonic BondsIonic Bonds • Transferred electrons• Formed between metals & nonmetals

• Metals = + cations w/full valence• Nonmetals = - anions w/full valence

• Opposing charges attract STRONGLY

Ionic CompoundsIonic Compounds • High melting pts• Good electrical conductors in solution

Page 6: Atomic Theory Practice

Ionic Bonding - Lewis Dot structuresIonic Bonding - Lewis Dot structures

http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html

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BONDINGBONDING

Non-polar CovalentNon-polar Covalent• e- shared equally• atoms w/similar

electronegativities

Polar CovalentPolar Covalent• e- shared UnUnequally• atoms w/different

electronegativities

Covalent BondsCovalent Bonds – shared electrons

http://iws.collin.edu/biopage/faculty/mcculloch/1406/outlines/chapter%202/chap02.html

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Covalent Bonding Covalent Bonding - Lewis Dot structures- Lewis Dot structures

http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html

Polar or Polar or Nonpolar?Nonpolar?

Polar or Polar or Nonpolar?Nonpolar?

Polar or Polar or Nonpolar?Nonpolar?

NonpolarNonpolar

NonpolarNonpolar

PolarPolar

Page 9: Atomic Theory Practice

Polarity in MoleculesPolarity in MoleculesNonpolarNonpolar Molecules

• Very little attraction between them• Generally gases @ room temp

• Ex: CO2

PolarPolar Molecules• Have dipoles (ends with opposite charges)• Electrons pulled toward more electronegative atom• Attraction between dipoles of adjacent molecules

• Ex: H2O

http://www.chem.umass.edu/genchem/whelan/class_images/Structure_of_Water.jpghttp://www.chem1.com/acad/webtext/states/interact.html

CO2

http://www.exo.net/~pauld/workshops/Greenhouse%20Effect/greenhouse.html

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VSEPR TheoryVSEPR Theory• VValence SShell

EElectron PPair RRepulsion• Outer shell e- pair up• Arrange themselves

as far apart from other pairs as possible since they repel other neg. charges

• Responsible for molecular shape

Sample Shapes

Bent

chemistry.gcsu.edu

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Bond LengthBond Length

Periodic Trend• as you move down group and right to left within a

period, bond length increases

• Same as atomic radius

• Double & triple bonds

are shorter than single

Radius & bond length increase

http://chemwiki.ucdavis.edu/Theoretical_Chemistry/Chemical_Bonding/Bond_Order_and_Lengths

http://www.chem.latech.edu/~upali/chem101/101MSJc8.htm

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Intermolecular ForcesIntermolecular Forces

Hydrogen Bonds• Formed between molecules whose atoms have

extremely different electronegativities• Most electronegative atoms: F, O, NF, O, N

bonded to• Least electronegative atom: HH

• Strong intermolecular force, causing high boiling points• Not nearly as strong as INTRAmolecular bonds

like covalent

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Bonding ReviewBonding Review

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Endergonic Endergonic (chem energy INTO your brain :)

Exercise #1Exercise #1

• In textbook, • Read p.275• Answer the following questions from p.276-77:

• MC 1,2,6,10• T/F 13,18• CM 22,24,26

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Chemical ReactionsChemical Reactions• Substances converted into NEW substances w/NEW

properties

Reactants – Reactants – What goes in

Products – Products – What comes out

Reactants Products

Glucose + Oxygen Carbon Dioxide + Water

C6H12O6 + O2 CO2 + H2O

C6H12O6 + 6O2 6CO2 + 6H2O

C6H12O6(s) + O2(g) CO2(g) + H2O(l)

WordsWords

FormulasFormulas

Balanced EquationBalanced Equation

Complete EquationComplete Equation

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Writing & Balancing Chemical Writing & Balancing Chemical EquationsEquations

• Going from word formula to balanced…1. Remember your naming rules!

a. Ionic compounds – cation (+) first then anion (-)

• # of + charges must equal # of - charges

• Ex: Sodium + Chlorine Sodium Chloride

Na+ + Cl- NaCl• Ex: Aluminum nitrate + Iron chloride Iron Nitrate + Aluminum Chloride

Al(NO3)3 + FeCl2 Fe(NO3)2 + AlCl3

a. Covalent compounds – use the number prefixes to indicate numbers of atoms

• Carbon + Chlorine Carbon Tetrachloride

C + 2Cl2 CCl4

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Ions & ChargesIons & ChargesCationsCations

+1+1• Group 1 atoms • Ammonium

• NH4+1

+2+2• Group 2 atoms

AnionsAnions-1-1

• Group 7 atoms • Chlorate = ClOChlorate = ClO33

-1-1

• Nitrate = NONitrate = NO33-1-1

• Hydroxide = OHHydroxide = OH-1-1

-2-2• Group 6 atoms• Sulfate = SOSulfate = SO44--22

• Carbonate = COCarbonate = CO33-2-2

-3-3• Group 5 atoms• Phosphate = POPhosphate = PO44

-3-3

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Naming & Writing Gases & AcidsNaming & Writing Gases & Acids

GasesGases• The name of the element followed by the word gas is always a

diatomic molecule• Ex: Oxygen gas = O2

• Ex: Chlorine gas = Cl2

• Ex: Hydrogen gas = H2

AcidsAcids• The name of an ion followed by the word acid means you add

the appropriate # of H’s in front of the ion• The # of H’s equals the - charge of the anion

• Ex: Hydrochloric acid = HCl• Ex: Sulfuric acid = H2SO4

• Ex: Phosphoric acid = H3PO4

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Types of Chemical ReactionsTypes of Chemical Reactions

1.1. Synthesis ReactionSynthesis Reaction

• aka direct combination reaction

• 2 or more reactants come together to form a single product

• A + B AB

• 2Na + Cl2 2NaCl

2.2. Decomposition ReactionDecomposition Reaction

• Single compound broken down into 2 or more smaller products

• AB A + B

• 2H2O 2H2 + O2

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3.3. Single Replacement ReactionSingle Replacement Reaction• Uncombined element takes the place of another

element within a compound• A + BX AX + B

• Mg + CuSO4 MgSO4 + Cu

• More active elements replace less active ones• Activity level shown in activity series• If uncombined element NOT more active, then

no reaction takes place

Types of Chemical ReactionsTypes of Chemical Reactions

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4. Double Replacement Reaction• Atoms or ions from 2 different compounds

replace each other• AX + BY AY + BX

• CaCO3 + 2HCl CaCl2 + H2CO3

Types of Chemical ReactionsTypes of Chemical Reactions