Presentation on theme: "Ionic Compounds. Metals Vs. NonMetals Metals Left of steps on Periodic Table 80 percent of elements are metals –Pie chart on page 36 Properties –Luster."— Presentation transcript:
Metals Vs. NonMetals Metals Left of steps on Periodic Table 80 percent of elements are metals –Pie chart on page 36 Properties –Luster –Conductivity –Malleable –Ductile NonMetals Right of steps 20 percent Properties –May lack luster –Do not conduct Except carbon –Brittle
Electron Configuration The properties of metals and nonmetals are greatly influenced by the electron configurations of atoms.
Ionic Compounds Atoms may gain or lose electrons thereby becoming ions. –Cation Positive Charge –AnionNegative Charge Why might a certain Ion gain rather than lose electrons?
Electron Configuration Number of electrons in the outermost shell is key. Few electrons Tend to lose them Close to full Shell Tend to gain Tendency towards stability
Compounds and Ionic Bonding A compound is a substance which is made of two or more kinds of atoms or ions which have joined together. Attractive force between positive and negative ions creates Ionic Compounds. NaCl Na+ Cl- The force of attraction between the positive and negative ions is known as an Ionic bond.
IMPORTANT When we talk about stability we are referring to the number of electrons in the valence shell.
Review Atom Ion Cation Anion Why does an atom lose or gain electrons? Predictions –Fluorine, Potassium, Lithium How many Chloride ions bond with Magnesium ions?
Forming Ionic Compounds (Salts) Ionic bonds form between METALS and NONMETALS when Electrons are transferred (lost or received). Columns 1,2,13 may transfer with columns 15,16,17.
Forming Ionic Compounds Atom gained one electron. It now has a negative charge. This atom lost one electron and now has a positive charge. Electrons get transferred as a result of energy input. This may also occur when materials are placed in solution. A variety of combinations are possible depending on the valence electron number.
Ionic Bonds An ionic bond is the attraction between a positively charged cation and a negatively charged anion.
Metals in columns 1, 2, 3 are electron donors. NonMetals in columns 5, 6, 7 receive Electrons.
Which Elements form Ionic Bonds? The central idea (for the 50 th time) is that electrons, one or more, are transferred between the outer shells of adjacent atoms. This Creates Ions/Charged Atoms. Metals and NonMetals. Certain Elements may donate or receive more than one electron. It can therefore bond with multiple elements.
Example #1 Na and Cl How many valence electrons does each atom have? Which atom will tend to Receive e-? Donate? What is the charge on each ion? What will the ratio between Na and Cl be?
Example #1 Na and Cl Sodium would lose one electron and become positively charged, while Chlorine would gain one electron becoming negatively charged. The positive/negative charge attraction would hold the two ions together.
Example #2 Mg and O How many valence electrons does each atom have? Which atom will tend to Donate e-? Receive? What is the charge on each ion? What will the ratio between Mg and O be?
Example #2 Mg and O The Magnesium would lose two electrons, becoming +2 charged and the Oxygen would gain the two electrons becoming -2 charged in the process. The negative/positive charge attraction (+2/-2) (four times as much as +1/-1) would hold the two ions together.
Example #3 Mg and Cl How many valence electrons does each atom have? Which atom will tend to gain e-? Donate? What is the charge on each ion? What will the ratio between Mg and Cl be?
Example #3 Mg and Cl The Magnesium would lose two electrons, becoming +2 charged and two chlorines (not one) would each gain one electron, each becoming -1 charged in the process. The three atoms would bond to each other by the positive/negative attraction between the ions.
Using the correct Name 1)K 2 S7) SrS 2) LiBr8) Al 2 O 3 3) Sr 3 P 2 9) MnO 4) BaCl 2 10) ZnO 5) NaBr11) ZnCl 2 6) MgF 2 12) Cu 2 O
Notation Ionic Notation 3 Na +1 1 PO 4 -3 Ionic Compound Formula NaCl CaCl 2 Na 3 (PO 4 )
Formulas Rules for Writing Formulas Metallic Donor is always written first. Nonmetallic Receiver is written second. Write the number of atoms required to balance the formula as subscripts after the element in compound. –NaCl –MgO –MgCl 2
HW: Write the Name of the Compound 1)MgS7) KBr 2) Ba 3 N 2 8) FeO 3) NaI9) SrF 2 4) Li 2 S10) CaO 5) Na 3 P11) Al 2 O 3 6) KCl12) Fe 2 O 3
HW: Write the Correct Formula 1)Magnesium Oxide 2) Lithium Bromide 3) Calcium Nitride 4) Sodium Sulfide 5) Copper (I) Sulfide 6) Copper (II) Sulfide
Practice Exercise #1 1.Which will donate, Which will receive? 2.How many will be donated/received? 3.Write the Ionic Notation of each. 4.Write the formula for each of the following. –Lithium Oxide –Potassium Chloride –Sodium Nitride –Calcium Chloride –Magnesium Sulfide –Barium Nitride –Aluminum Fluoride –Aluminum Oxide –Aluminum Nitride
Diagramming Ionic Compounds Lewis Structures –Diagram valence shell. Place valence electrons around nucleus as they would be according to the octet rule
Practice Exercise #4 Write out the Ionic Notation, Formula and Names of the following ionic compounds: –Li and F- Na and CO 3 -2 –Na and S- Li and OH -1 –K and Br- NH 4 +1 and Cl –Rb and O- Ca and SO 4 -2 –Ca and Cl- NH 4 +1 and OH -1 –Mg and SO 3 -2 - Na and CN -1 – Al and NO 3 -1 - NH 4 +1 and SO 4 -2
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