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.
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
Identity and Change Unit
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.
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.
Magnetic stir plate
A charged particle (either a single atom or a molecule)
A positively charged particleNa+ H+ Ca2+ Cu2+ NH4+
A negatively charged particleCl- O2- OH- NO3- SO42-
An electron in the outermost energy level for an atom.
The electrons that interact when atoms form bonds.
H Li Na
C N F
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)
Sodium atom Sodium ion
11 protons11 protons
11 electrons 10 electrons
Chlorine atom Chlorine ion
17 protons17 protons
17 electrons 18 electrons
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
Identify the number of valence electrons in each of the following elements:
Be B N F
Mg Al P Cl
Ca As Br
A graphic representation of the number and placement of valence electrons for an atom or ion.
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.
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
Draw dot diagrams for the following anions:
N3- O2- F-
P3- S2- Cl-
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.
A chemical bond resulting from the transfer of electrons from one bonding atom to another.
A bond involving ions.
aluminum oxideNomenclature: Names to Formulas
Al2O3Nomenclature: Names to Formulas
copper (I) bromide
iron (II) sulfide
lead (II) oxide
copper (I) sulfide
mercury (I) chloride
nickel (II) phosphateNomenclature: Names to Formulas
Ni3(PO4)2Nomenclature: Names to Formulas
Sum of the atomic masses of all atoms represented in a chemical formula, represented either in atomic mass units (amu) or g
H2O2Nomenclature: Formulas to Names
sodium hydrogen carbonate
33.996Nomenclature: Formulas to Names
Cu2ONomenclature: Formulas to Names
copper (II) hydroxide
nickel (II) carbonate
nickel (II) chloride
iron (II) sulfate
iron (III) sulfate
lead (II) nitrate
mercury (I) chloride
mercury (II) chloride
copper (I) oxideNomenclature: Formulas to Names
Water + glucose
Water + starch
Water + sodium chloride
Water + sodium hydroxide
Water + copper (II) nitrate
Water + copper (II) nitrate + sodium hydroxide
A system designed by American chemist
to demonstrate the interactions of valence electrons in the formation of compounds.
Cl C Cl
Draw Lewis Structures for the following ionic compounds:
NaCl KF RbBr CsI
MgO CaS Na2O K2S
AlP Mg3N2 Na3N KH