notes – chemical bonding and electron transfer assign # 30 pt
TRANSCRIPT
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Notes – Chemical Bonding and Electron Transfer
Assign # 30 pt.
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Chemical Bonding
• Chemical Bonds – Chemical forces which hold atoms together and form complete electrons shells
• Atoms of elements will transfer or share electrons to reach the stable octet number.
Inert (Noble) Gases have 8 valence electrons (2 for He) and are stable
Nonmetals –Groups 5a to 7a will gain electrons to become stable
Metals – Groups 1a to 3a will lose electrons to become stable
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Chemical Bonds – Chemical forces which hold atoms together and form complete
electrons shells• Ionic Bond – Positive (+) and
negative (-) ions attract – formed by the transfer of valence electrons.Na 11p+ 11p+
11e- 10e- = +1 Na
Cl 17p+ 17p+17e- 18e- = -1 Cl
Na +1 + Cl-1 = NaCl o
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
Na = 11 p+ Na = 11 p+ 11 e - 10 e-
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
Cl = 17 p+ Cl = 17 p+ 17 e - 18 e-
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Ionic Bonds
Ion – is an atom or group of atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
Na +1 + Cl-1 = NaCl o
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Ionic bond
• Atoms which lose electrons become positive (cations)
Lose 1 = +1Lose 2 = +2Lose 3 = + 3• Atoms which gain electrons
become negative (anions)Gain 1 = - 1Gain 2 = - 2Gain 3 = -3
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Ionic Bond
• Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions
• Na + plus Cl - combining to form NaCl is an example
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Ionic Bond
• Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions
• Na + plus Cl - combining to form NaCl is an example
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Ionic Bond
• Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions
• Na + plus Cl - combining to form NaCl is an example
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Ionic Bond
• Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions
• Na + plus Cl - combining to form NaCl is an example
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Ionic Bond
• Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions
• Na + plus Cl - combining to form NaCl is an example
• A compound consisting of positive and negative ions such as NaCl = sodium chloride is an Ionic Compound
Sodium Chloride
Ionic Compound
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Table Salt
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Oxidation – Reduction Reactions
Reduction – Any reaction in which a reactant can be considered to gain one or more electrons.
Elements or ions which lose electrons are said to be reduced.
Cu 2+ + 2e- = Cu Copper II ion Copper metal
Reduction Reaction. Copper ions are reduced
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Oxidation – Reduction Reactions
Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons.
Elements or ions which gain electrons are said to be oxidized.
Cu = Cu 2+ + 2e- Copper metal Copper II ion
Oxidation Reaction. Copper ions are oxidized
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Oxidation – Reduction Reactions
Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons.
Elements or ions which gain electrons are said to be oxidized.
Cu = Cu 2+ + 2e- Copper metal Copper II ion
Oxidation Reaction. Copper ions are oxidized
Oil Rig : Oxidation is Loss (of electrons), Reduction is Gain (of electrons)
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Oxidation – Reduction Reactions
Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons.
Elements or ions which gain electrons are said to be oxidized.
Cu = Cu 2+ + 2e- Copper metal Copper II ion
Oxidation Reaction. Copper ions are oxidized
Oil Rig : Oxidation is Loss (of electrons), Reduction is
Gain (of electrons)Cu + O2 = 2CuO
Copper is OxidizedOxygen is Reduced
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Oxidation – Reduction Reactions
Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons.
Elements or ions which gain electrons are said to be oxidized.
Cu = Cu 2+ + 2e-
Copper metal Copper II ionOxidation Reaction. Copper ions are oxidized
Oil Rig : Oxidation is Loss (of electrons), Reduction is Gain
(of electrons)Cu + O2 = 2CuO
Copper is OxidizedOxygen is ReducedCopper loses electronsOxygen gains electrons
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• Metals can be changed to ions by oxidation.
• Mg Mg2+ + 2e-
• Metallic ions can be changed to metals by reduction.
• Al3+ + 3e- Al
Oxidation – Reduction Reactions
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• Metals and Metal ions will react in a Redox, Reduction-Oxidation reaction.
• The more active metal will react with a less active ion in a replacement reaction
• Cu + Ag+ Ag + Cu+
Cu is oxidized, Ag+ is reducedCu loses an e-, Ag gains an e-
Oxidation – Reduction Reactions
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Metallic bonding
• Metal atoms combine in regular patterns in which valence electrons are free to move from atom to atom.
• Most metals have from 1 to 3 valence electrons and are positive ions.
• Metal ions are held in place by a metallic bond an attraction between a positive metal ion and the many electrons surrounding it.
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Metallic bonding
• Most metals have from 1 to 3 valence electrons and are positive ions.
• Metal ions are held in place by a metallic bond an attraction between a positive metal ion and the many electrons surrounding it.
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Metal Properties
• Metals properties are attributed to the “sea of electrons” flowing over the positive ions
• Malleable and ductile – metal’s positive ions are attracted to electrons and can slide into different positions
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Metal Properties
• Luster – When light strikes the valence electrons they absorb it than give it off again
• Electrical and Thermal conductivity – valence electrons move freely and cause electric current to flow or heat to flow easily from hot to cold
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Covalent Bonding
• Covalent Bond – the chemical bond formed when atoms share electrons
• The force holding them together is the attraction of the nucleus and the shared electrons
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Covalent Bonding
• Covalent Bond – the chemical bond formed when atoms share electrons
• The force holding them together is the attraction of the nucleus and the shared electrons
• Usually forms between atoms of nonmetals
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Covalent Bonding• Covalent Bond – the
chemical bond formed when atoms share electrons
• The force holding them together is the attraction of the nucleus and the shared electrons
• Usually forms between atoms of nonmetals
• The neutral group of atoms joined by covalent bonds is called a molecule
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Covalent Bonding
• The neutral group of atoms joined by covalent bonds is
called a molecule• Molecular
compounds is a compound composed of covalently bonded molecules
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Covalent bonding – Sharing of valence electrons to fill electron shells
• Follows octet rule, except for H and He
• Common elements-
H, C, N, 0
Lines show shared electrons H O
H
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H20 – Molecular formula
H OH
- Structural formula – shows the number and position of atoms
O N C
O N C
Show the bonds formed when these atoms combine with Hydrogen (H. )
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H20 – Molecular formula
H OH
- Structural formula – shows the number and position of atoms
Show the bonds formed when these atoms combine with each other
H + H =
Cl + Cl =
Br + Br =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons
O + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons
O + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons
O + O =
O + C + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons
O + O =
O + C + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons
O + O =
O + C + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons
O + O =
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Covalent Bonding
• Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons
• Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons
O + O =
O + C + O =
N + N =
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Covalent Bonding
•Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons
N + N =
C + O =
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Table SaltNaCl- Sodium Chloride
Sugar - glucose
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• Abbreviated form of compound showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound.
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• Examples-• NaCl• MgCl2
• Li2Cl
• Al2O3
• K2SO4
Chemical formulas
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Chemical formulas –• Abbreviated form of compound
showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Examples-• NaCl =• MgCl2
• Li2Cl
• Al2O3
• K2SO4
Types of Matter
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Chemical formulas –• Abbreviated form of compound
showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Examples-• NaCl = Sodium Chloride• MgCl2
• Li2Cl
• Al2O3
• K2SO4
Types of Matter
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Chemical formulas –• Abbreviated form of compound
showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Examples-• NaCl = Sodium Chloride• MgCl2 =Magnesium
Chloride• Li2Cl
• Al2O3
• K2SO4
Types of Matter
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Chemical formulas –• Abbreviated form of compound
showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Examples-• NaCl = Sodium Chloride• MgCl2 =Magnesium
Chloride• Li2Cl = Lithium Chloride
• Al2O3
• K2SO4
Types of Matter
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Chemical formulas –• Abbreviated form of compound
showing the element symbols and ratio of atoms
• A subscript shows you the number and ratio of atoms in a compound
• Ex: Al2O3 = 2 aluminum and 3 oxygen
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Examples-• NaCl = Sodium Chloride• MgCl2 =Magnesium
Chloride• Li2Cl = Lithium Chloride
• Al2O3 = Aluminum Oxide
• K2SO4
Types of Matter
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Chemical formulas –
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Ions that are made of more than one atom are called polyatomic ions.
• Ex: SO4 = sulfate
• Examples-• NaCl = Sodium Chloride• MgCl2 =Magnesium
Chloride• Li2Cl = Lithium Chloride
• Al2O3 = Aluminum Chloride
• K2SO4 = Potassium Sulfate
Types of Matter
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Chemical formulas –
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Ions that are made of more than one atom are called polyatomic ions.
• Ex: SO4 = sulfate
• Examples-• LiCl =• K2S =
• CaF2 =
• MgO2 =
• Na2PO4 =
Types of Matter
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Chemical formulas –
• When naming ionic compounds the positive ion comes first, followed by the name of the negative ion
• Ions that are made of more than one atom are called polyatomic ions.
• Ex: SO4 = sulfate
• Examples-• LiCl = Lithium Chloride• K2S = Potassium Sulfide
• CaF2 = Calcium Flouride
• MgO2 = Magnesium Oxide
• Na2PO4 = Sodium Phosphate
Types of Matter
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Table SaltNaCl- Sodium Chloride
Sugar - glucose