Forming Chemical Bonds - Mister Chemistry
Transcript of Forming Chemical Bonds - Mister Chemistry
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Forming Chemical Bonds
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Why do atoms form chemical bonds ?
so that the system can achieve the lowest possible potential energy
H • H•
Example covalent bonding in H2
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Distance of separation between atoms
0
Pote
ntia
l ene
rgy
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The subscript to the right of the symbol of an element tells the number of atoms of that element in one molecule of the compound.
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Atoms, Molecules, and Ions
Chemical Formulas
CO2
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C O2
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Atoms, Molecules, and Ions5
The subscript to the right of the symbol of an element tells the number of atoms of that element in one molecule of the compound.
Chemical Formulas
the number 1 is not used as a subscript
1
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Ions and Ionic Compounds
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Ionic compounds
Any compound when melted that conducts electricity is considered ionic
NaCl( s) is made up of Na+ and Cl- ions
Example : NaCl(s) NaCl( l)
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When electrons are removed from or added to a neutral atom or molecule, a
charged particle called an ion is formed.
Ions
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Positively charged ions are calledcations
Negatively charged ions are calledanions
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Ionic Bonds
especially prevalent in compounds formed between group 1A and 2A elements with group 6A and 7A elements.
between Elements with the biggest difference in electronegativity
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Ionic Bonds
especially prevalent in compounds formed between group 1A and 2A elements with group 6A and 7A elements.
between Elements with the biggest difference in electronegativity
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Electronegativity
measure of an element to attract electrons toward itself when bonded to another element
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Electronegativity
Increases from left to right in periodic table.
Decreases going down a group.
Fluorine is the most electronegative element.
Francium is the least electronegative element.
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Periodic Properties
of the Elements
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Properties of Metal, Nonmetals,and Metalloidselectronegativity
increasingelectronegativity
decreasing
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Periodic Properties
of the Elements
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Properties of Metal, Nonmetals,and Metalloids
least electronegative
most electronegative
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Pauling Electronegativity Scale
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Metals Nonmetals
In chemical reactions metals tend to lose electrons to nonmetals
Metalloids
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metalsgood conductors of heat and electricity
malleable
ductile
lustrous
tend to lose electrons in chemical reactions
nonmetalspoor conductors
brittle
tend to gain electrons in chemical reactions
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Specific Groups
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Main groupsgroup numbers identified by suffix A
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Main group metalsAlkali metals Alkaline earth metals
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NonmetalsHalogens Noble gases
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transition metals
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Periodic Properties
of the Elements
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Metals versus Nonmetals• Metals tend to form cations. • Nonmetals tend to form anions.
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Ionic compounds are usually formed between metals and nonmetals.
Ionic and Molecular Compounds
Molecular compounds are usually formed between two nonmetals.
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Atoms vs Ions
Na: 11 protons; 11 electrons
Cl: 17 protons; 17 electrons
Cl–: 17 protons; 18 electrons
–
Na+: 11 protons; 10 electrons
+
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H-
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Ionic Bonding
electrostatic attraction between oppositely charged ions
–+
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discrete molecules are not present, so ionic compounds are represented by their empirical formulas
Ionic Compounds
some times referred to as formula units
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Empirical formula tells us which elements are present and the simplest whole-number ratio of their atoms.
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the ions are packed together to maximize (+) (-) attractions and minimize (+) (+) and (-) (-) repulsions
Solid structure of LiF
Crystal lattice
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• compounds are electrically neutral
Writing Formulas
• The subscripts in the chemical formula must be in smallest whole numbers
• The sum of the positive charges of the cations must equal the sum of the negative charges on the anions.
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Writing Formulas
Mg Ngroup II A group VA
• find the charge on the ions
2 + 3 -
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Writing Formulas
Mg N2 + 3 - Mg3N2
Mg2+
Mg2+
Mg2+
3N3-
N3-2
3(2+) = +6 -6 = 2(3-)
• compounds are electrically neutral
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Writing Formulas
Mg N2 + 3 - Mg3N2
Mg2+
Mg2+
Mg2+
N3-
N3-3 2
3(2+) = +6 -6 = 2(3-)
• subscripts in smallest whole numbers
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Molecules:Atoms in Combination
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Molecule —is an aggregate of at least two atoms in a definite arrangement held together by chemical forces.
Definition
structurebonds
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Chemical FormulasExpress the composition of molecules and ionic compounds in terms of the symbols for the elements they contain.
Empirical formula tells us which elements are present and the simplest whole-number ratio of their atoms.Molecular formula gives the exact number of atoms each element in the compound
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Atoms, Molecules, and Ions
Chemical Formulas
Molecular compounds are composed of molecules and almost always contain only nonmetals.
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A molecule is not necessarily a compound.
ExampleH2 O2 Cl2
A compound is not necessarily molecular.
ionic compounds
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Atoms, Molecules, and Ions
Diatomic Molecules
• These seven elements occur naturally as molecules containing two atoms: – Hydrogen – Nitrogen – Oxygen – Fluorine – Chlorine – Bromine – Iodine
O2
N2
F2
Cl2Br2
I2
H2
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Hydrogen
the stable form of the element is diatomic a molecule H2
ball-and-stick model space-filling model
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is a polyatomic molecule (contains three atoms connected in the order HOH).
Water (H2O)
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Atoms, Molecules, and Ions
Types of Formulas
• Structural formulas show the order in which atoms are bonded.
• Perspective drawings also show the three-dimensional array of atoms in a compound.
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Atoms, Molecules, and Ions
Common Cations
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Atoms, Molecules, and Ions
Common Anions