Chemical Names and Formulas 6.1 Introduction to Chemical Bonding 6.2 Representing Chemical Compounds...
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Transcript of Chemical Names and Formulas 6.1 Introduction to Chemical Bonding 6.2 Representing Chemical Compounds...
Chemical Names and Formulas
6.1 Introduction to Chemical Bonding6.2 Representing Chemical Compounds6.3 Ionic Charges6.4 Ionic Compounds6.5 Molecular Compounds and Acids6.6 Naming and Formula Writing
6.1 Objectives Distinguish between ionic and molecular
compounds Define cation and anion, relate them to metal
and non-metal
metal/cation nonMetal/anion
6.1 Vocabulary Molecule Molecular compound Ions Cations Anions Ionic compounds
Introduction to Chemical Bonding
Molecules and Molecular Compounds Tend to have low boiling and melting points May be gases or liquids at room temperature (RT) Are composed of non-metals, CO2
Ions and Ionic Compounds, (+) and (-) Have balanced charges, 2(+) must have 2(-) Have high boiling and melting points, (solid at RT) Are composed of metals and non-metals
(combined)
Ions: Symbols and Names
Cations: these are metals that lose electrons When you lose a (-) you become more positive If Potassium (K) loses 1 electron it becomes K+1
Example: (19+ and 19–) changes to (19+ and 18-) Anions: these are nonMetals that gain electrons
When you gain a (-) you become more negative If Bromine (Br) gains one electron it becomes Br-1
Example: (35+ and 35-) changes to (35+ and 36-) Anions change their suffix to –ide, (Bromine to
Bromide)
Characteristics of CompoundsCharacteristic Molecular
CompoundIonic Compound
Representative Unit Molecule Formula Unit
Type of Elements nonMetals Metal and nonMetal
Physical State Solid, liquid , or Gas Solid
Melting Point Low, (below 300 C) High, (above 300C)
Questions What is the symbol and name for an Oxygen
atom that has gained two electrons? O2- and Oxide What is the symbol and name for an Iron atom
that has lost two electrons? Fe2+ and Iron (II)
Definitions A Molecule is the smallest electrically neutral
unit of a substance A Molecular compound are combinations of
atoms Ions are charged atoms or molecules Cations are positively charged (+) Anions are negatively charged (-) Ionic compounds combine the (+) and (-)
6.2 Objectives Distinguish among chemical formulas,
molecular formulas, and formula units Use experimental data to show that a
compound obeys the law of definite proportions
Vocabulary Chemical formula Molecular formula Formula unit Law of Definite Proportions Law of Multiple Proportions
Formula Unit is a crystal
HONClBrIF
Diatomic Molecules, (exist as two bonded atoms) (H) Hydrogen as H2
(O) Oxygen as O2
(N) Nitrogen as N2
(Cl) Chlorine as Cl2
(Br) Bromine as Br2
(I) Iodine as I2
(F) Fluorine as F2
Counting Atoms and Assigning Mass When elements react to form
compounds, they react in defined, whole-number ratios. The experiments that Dalton and others performed showed that reactions are not random events; they proceed according to precise and well-defined formulas.
Water, for example, is always made up of two parts hydrogen and one part oxygen. The chemical formula of a compound is written by listing the symbols of the elements together, without any spaces between them. If a molecule contains more than one atom of an element, a number is subscripted after the symbol to show the number of atoms of that element in the molecule. Thus the formula for water is H2O, never HO or H2O2.
Questions How are the images different? In every sample of Carbon Monoxide the mass
ratio is 3:4 for the mass of Carbon : Oxygen. In sample 1: Carbon is 9 grams and Oxygen is ____ In sample 2: Carbon is _____and Oxygen is 8 grams
Definitions
A Chemical formula shows the kind and number of atoms in a representative unit
A Molecular formula shows the kind and number of atoms in a molecule
A Formula unit is the lowest whole number ratio in a compound, when ions come together to form a crystal
Law of Definite Proportions: the masses of the elements in a compound always conform to a ratio
Law of Multiple Proportions: different compounds may have different ratios of the same elements
6.3 Objectives Use the Periodic Table to determine the
charge of an ion Define a polyatomic ion Name the most common examples of
polyatomic ions
Vocabulary Monoatomic ions Polyatomic ions
The Mono-Atomic Ions
See the table on page 143 for the Representative Elements
See the table on page 144 for some Transition Metal Elements
Some Transition Metal Ions
Complexes may be quite colorful The paint industry uses transition metal ions
to provide color
Poly-Atomic Ions
Ammonium ion is positive (+) Nitrate ion is negative (-) In each case there are multiple atoms acting
as a tightly bound unit The table on page 147 provides a good list
Questions
What is the charge on a Potassium atom that has changed to an ion?
What is the charge of a Bromine atom that has changed to an ion?
Using page 147, what is the charge of Sulfite? What is the charge of Iron (III)?
How would you write an ion of Cobalt (II)? What is the name of Sn+4 ?
Definitions Monoatomic ions are ions consisting of only
one atom Cation: Li+1
Anion: Br-1
Polyatomic ions are tightly bound groups of atoms that behave as a unit and carry a charge Cation: NH4
+1
Anion: Cr2O7-2
6.4 Objectives Apply the rules for naming and writing
formulas for binary compounds Apply the rules for naming and writing the
formulas for ternary ionic compounds
Vocabulary Binary compounds Ternary compounds
How to write a chemical formula
Start by identifying the types of atoms Hydrogen and Oxygen
Count the atoms of each type Two H and One O leads to the formula H2O
Naming a binary ionic compound
Determine the positive ion, in this case Sodium+
Determine the negative ion, in this case Chlorine-
Determine the charges (+) and (-), both are 1 The positive (cation) is first, then the anion Sodium Chloride is NaCl and has no charge
Naming a ternary ionic compound
Notice the green ball, (Mg+2), and the ball that is red/white, (OH-), the ratio is 1:2 or Mg(OH)2
Magnesium Hydroxide
Definitions Binary compounds are composed of two
elements NaCl
Ternary compounds are composed of three different elements CaCO3
6.5 Objectives Apply the rules for naming and writing
formulas for binary molecular compounds Name and write formulas for common acids
Binary molecular compounds
Prefixes for naming binary molecular:mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa-8 nona- 9
deca- 10 - diNitrogen tetraHydride, (N2H4)
Naming common acids
(aq) means it is in water Acids break apart in water Six acids are commonly
used, (see the chart at left) There are rules for naming
acids, (hydro- and –ic acids)
6.6 Objectives Use the flowchart in Fig. 6.21 to write the
name of a compound when given its chemical formula
Use the flowchart in Fig. 6.23 to write a chemical formula of a compound when given its name