Chemistry dma
Download
1 / 29

chemistry dma - PowerPoint PPT Presentation


  • 282 Views
  • Updated On :

Chemistry DMA. Write out the abbreviated electron configuration for the following elements: Li [He]2s 1 O Ne Na S [Ne]3s 2 3p 4 Ar K Se Kr [Ar]4s 2 3d 10 4p 6 Rb Te Xe Cs [Xe]6s 1 Po Rn . Ions. Identity and Change Unit. Soluble/Insoluble.

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about 'chemistry dma' - bernad


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
Chemistry dma l.jpg
Chemistry DMA

Write out the abbreviated electron configuration for the following elements:

Li [He]2s1 O Ne

Na S [Ne]3s23p4 Ar

K Se Kr [Ar]4s23d104p6

Rb Te Xe

Cs [Xe]6s1 Po Rn


Slide2 l.jpg

Ions

Identity and Change Unit


Soluble insoluble l.jpg
Soluble/Insoluble

A soluble substance can be dissolved.

If something will not dissolve, it is insoluble. If two or more chemicals are mixed in a solution and a solid appears, the solid is insoluble. In this case, the solid is called a precipitate.


Solution l.jpg
Solution

Solutions are mixtures of solvents and solutes.

Solvents are substances that dissolve – they cause another substance to disperse, disintegrate, break apart.

Solutes are substances that dissolve in solvents. Solutes break apart in solvents.


Diagram the demo set up l.jpg
Diagram the demo set-up

Light bulb

Beaker

Magnetic stir plate


Slide6 l.jpg

Ion

A charged particle (either a single atom or a molecule)

Cation

A positively charged particleNa+ H+ Ca2+ Cu2+ NH4+

Anion

A negatively charged particleCl- O2- OH- NO3- SO42-


Valence electron l.jpg
Valence Electron

An electron in the outermost energy level for an atom.

The electrons that interact when atoms form bonds.

H Li Na

C N F


Valence electrons l.jpg
Valence electrons

The s and p electrons in the outermost primary energy level.

There are 2 valence electrons for the 1st primary energy level. (Period 1)

There are 8 valence electrons in every other primary energy level. (Periods 2-7)


Bohr models of atoms and ions l.jpg
Bohr Models of Atoms and Ions

Sodium atom Sodium ion

11 protons11 protons

Na Na

11 electrons 10 electrons

Chlorine atom Chlorine ion

17 protons17 protons

Cl Cl

17 electrons 18 electrons


Ionic bond l.jpg
Ionic bond

A bond formed by the attraction between a cation and an anion. Ionic bonds create an ionic compound. Although the cations and anions they are made from have positive and negative charges, ionic compounds have a balance of positive and negative charges, and hence, no net charge.

Na Na Cl Cl


Valence electrons practice l.jpg
Valence Electrons Practice

Identify the number of valence electrons in each of the following elements:

Be B N F

Mg Al P Cl

Ca As Br

Sr I


Dot diagram l.jpg
Dot diagram

A graphic representation of the number and placement of valence electrons for an atom or ion.


Vsepr theory l.jpg
VSEPR theory

Valence

Shell

Electron

Pair

Repulsion

A theory based on experimental observations that suggests valence electrons occur in pairs that separate as far as possible three dimensionally from other pairs in the same valence shell.


Dot diagram practice l.jpg
Dot diagram practice

Draw dot diagrams for the following elements:

Li B N F Ne

Na Si S Ar

Ca Ga Ge As Br

Rb Sn Te Xe

Ba Tl Bi Po At


Dot diagram practice15 l.jpg
Dot diagram practice

Draw dot diagrams for the following anions:

H-

N3- O2- F-

P3- S2- Cl-

Se2- Br-

I-


Ionic compounds l.jpg
Ionic compounds:

Chemical combinations of two or more different elements in a fixed ratio.

Contain ions which are attracted to each other due to opposite electrical charges.

Have no net charge due to balancing of the charges on the cation (+) and anion (-).

Ionic compounds are generally formed between a metallic cation and an anion.


Ionic bond17 l.jpg
Ionic bond:

A chemical bond resulting from the transfer of electrons from one bonding atom to another.

A bond involving ions.

NaClNa+Cl-


Nomenclature names to formulas l.jpg

sodium chloride

sodium bromide

potassium iodide

rubidium bromide

calcium sulfide

strontium oxide

sodium sulfide

sodium nitride

calcium chloride

barium iodide

aluminum chloride

aluminum oxide

Nomenclature: Names to Formulas


Nomenclature names to formulas19 l.jpg

NaCl

NaBr

KI

RbBr

CaS

SrO

Na2S

Na3N

CaCl2

BaI2

AlCl3

Al2O3

Nomenclature: Names to Formulas


Nomenclature names to formulas20 l.jpg

copper (I) chloride

copper (I) bromide

iron (II) sulfide

lead (II) oxide

calcium carbonate

strontium sulfate

copper (I) sulfide

mercury (I) chloride

calcium nitrate

barium hydroxide

aluminum phosphate

nickel (II) phosphate

Nomenclature: Names to Formulas


Nomenclature names to formulas21 l.jpg

CuCl

CuBr

FeS

PbO

CaCO3

SrSO4

Cu2S

Hg2Cl2

Ca(NO3)2

Ba(OH)2

AlPO4

Ni3(PO4)2

Nomenclature: Names to Formulas


Molecular weight l.jpg
Molecular Weight

Sum of the atomic masses of all atoms represented in a chemical formula, represented either in atomic mass units (amu) or g


Nomenclature formulas to names l.jpg

KI

MgS

NaOH

KNO3

CaSO4

NaClO4

NaHCO3

Zn(NO3)2

SrCl2

Ba3(PO4)2

(NH4)2Cr2O7

H2O2

Nomenclature: Formulas to Names


Nomenclature formulas to names24 l.jpg

potassium iodide165.998

magnesium sulfide56.370

sodium hydroxide

39.997

potassium nitrate

94.102

calcium sulfate

136.139

sodium perchlorate78.442

sodium hydrogen carbonate

161.998

zinc nitrate

127.394

strontium chloride158.526

barium phosphate

601.930

ammonium dichromate

252.062

hydrogen peroxide

33.996

Nomenclature: Formulas to Names


Nomenclature formulas to names25 l.jpg

CuO

Cu(OH)2

NiCO3

Al(NO3)3

NiCl2

AgC2H3O2

FeSO4

Fe2(SO4)3

Pb(NO3)2

Hg2Cl2

HgCl2

Cu2O

Nomenclature: Formulas to Names


Nomenclature formulas to names26 l.jpg

copper (II) oxide

copper (II) hydroxide

nickel (II) carbonate

aluminum nitrate

nickel (II) chloride

silver acetate

iron (II) sulfate

iron (III) sulfate

lead (II) nitrate

mercury (I) chloride

mercury (II) chloride

copper (I) oxide

Nomenclature: Formulas to Names


Slide27 l.jpg

Distilled Water

Water + glucose

Water + starch

Water + sodium chloride

Water + sodium hydroxide

Water + copper (II) nitrate

Water + copper (II) nitrate + sodium hydroxide


Lewis structures l.jpg
Lewis structures

A system designed by American chemist

Gilbert Lewis

to demonstrate the interactions of valence electrons in the formation of compounds.

F

Cl C Cl

F


Ionic compounds lewis structures l.jpg
Ionic Compounds: Lewis Structures

Draw Lewis Structures for the following ionic compounds:

NaCl KF RbBr CsI

MgO CaS Na2O K2S

AlP Mg3N2 Na3N KH


ad