Chemical Bonding-Focus Ionic! Bonding: Ionic, Metallic, & Covalent.
Unit 10 Ionic Bonding
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Transcript of Unit 10 Ionic Bonding
![Page 1: Unit 10 Ionic Bonding](https://reader034.fdocuments.net/reader034/viewer/2022051414/55a429251a28aba3038b4845/html5/thumbnails/1.jpg)
Ionic Bonding
Unit 10
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Valence Electrons
• Valence electrons are the electrons in the outermost s and p-orbitals that can be involved in chemical reactions.
1s orbital is not involved
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Valence Electrons
• Valence electrons are the electrons in the outermost s and p-orbitals that can be involved in chemical reactions.
1s orbital is not involved
Outer octet of 2s and 2p orbitals are involved
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Ions
Cation Positively Charged Atom
(loses electrons)
K+1
Pronounced CAT-ion
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Ions
Cation Positively Charged Atom
(loses electrons)
K+1
Anion Negatively Charged Atom
(gains electrons)
Cl-1
Pronounced AN-ion
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Ions
Cation Positively Charged Atom
(loses electrons)
K+1
Anion Negatively Charged Atom
(gains electrons)
Cl-1
Ionic Bonding occurs when a cation gives electrons to an anionand the atoms become attracted to each other due to the opposite charges.
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Ionic Bonds
• Sodium has one valence electron it wants to lose
• Chlorine has 7 valence electrons, so it wants to gain one more to make it to eight.
·Na Cl :
:
·
:
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Ionic Bonds
• The Sodium atom donates it’s one valence electron to Chlorine.
·Na Cl :
:
·
:
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Ionic Bonds
• This means Na has the electron configuration of the noble gas before it, which is Neon
• Sodium’s electron configuration is now written as [Ne]+
·Na+1 Cl-1:
:
·
:
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Ionic Bonds
• Chlorine now has the electron configuration of the noble gas after it, which is Argon.
• Chlorine’s electron configuration is now written as [Ar]-
·Na+1 Cl-1:
:
·
:
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Ionic Bonds
• Sodium and Chloride are now ionically bonded to form a new compound known as sodium chloride (NaCl).
• This is known to most of us as Table Salt.
Na Cl ::
::
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Ionic Bonds
• Now each sodium is positively charged and each chlorine is negatively charged.
• They are attached because opposite charges attract electrostatically.
• However, together they balance each other out.
Na+1 -1
Cl ::
::
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Ionic Bonds
• But, the positive charge, does attract other negatively charged molecules, such as other chlorine ions
• The same holds true for negatively charged chlorine ions attracting other positive ones
Na+1 -1
Cl ::
::-1
Cl ::
::
Na+1
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Ionic Bonds
• Soon, they all begin to line up
Na+1 -1
Cl ::
::
-1Cl ::
::
Na+1
Na+1 Cl ::
::
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Ionic Bonds
• Soon, they all begin to line up
• This then forms crystals of salt
Na+1 -1
Cl ::
::
-1Cl ::
::
Na+1
Na+1
Cl ::
::
-1Cl ::
:: Na
+1-1
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Ionic Bonds
• Soon, they all begin to line up
• This then forms crystals of salt
Na+1 -1
Cl ::
::
-1Cl ::
::
Na+1
Na+1
Cl ::
::
-1Cl ::
::
Na+1-1
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Ionic Bonds
• Bonding that involves a transfer of electrons.
• Positively and negatively charged atoms (ions) result from this transfer
• The resulting positive and negative charged atoms are “attracted” to each because of their opposite charges.
Na+ Cl-
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Solvents and Solutions
• Because ionic molecules have positive and negative atoms, they can be pulled apart by other substance with positive and negative charges.
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Solvents and Solutions• One example is dissolving salt into water
• Water molecules have positive ends near the hydrogens and negative ends near the oxygen.
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Solutions
• Since all of the ions are evenly dispersed and dissolved in the water, it makes a solution of salt water.
• This solution is transparent.
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Reforming Crystals• When the water evaporates, the positive Na
ions and the negative Cl ions come back together again!
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So, Who Makes Ions Anyways?
• It all depends on how many valence electrons they have and what they need to get to noble gas configuration.
Secret Question #1: How many valence electrons does Aluminum have?
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So, Who Makes Ions Anyways?
• It all depends on how many valence electrons they have and what they need to get to noble gas configuration.
Secret Question #1: How many valence electrons does Aluminum have?
Answer: 3
Secret Question #2: What ionic charge will it have to become noble gas configuration?
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So, Who Makes Ions Anyways?
• It all depends on how many valence electrons they have and what they need to get to noble gas configuration.
Secret Question #1: How many valence electrons does Aluminum have?
Answer: 3
Secret Question #2: What ionic charge will it have to become noble gas configuration?
Answer: Al-3
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Alkali Metals
Charge: +1
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Alkaline Earth Metals
Charge: +2
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Boron Family
Charge: +3
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Carbon Family
Do not usually make ions, but could be +4 or -4
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Nitrogen Family
Charge: -3
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Oxygen Family
Charge: -2
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Halogens
Charge: -1
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Noble Gas Family
Do not have ions, because they already have full orbitals
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Transition Metals
A variety of positive ions from +1 to +7Why and how is beyond the scope of this course
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Polyatomic Ion
• Polyatomic ions are ions that have multiple atoms attached to each other, but as a unit have a net charge.
• Sulfate (SO4-2) is an example.
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Polyatomic IonsAnions
Acetate CH3COO−
Bicarbonate (hydrogen carbonate) HCO3-
Carbonate CO3-2
Cyanide CN−
Hydroxide OH−
Nitrate NO3-
Phosphate PO4-3
Sulfate SO4-2
Sulfite SO3-2
Cations
Ammonium NH4+
Hydronium H3O+
Mercury(I) Hg2+2
State −1 +1 +3 +5 +7
Anion name chloride hypochlorite chlorite chlorate perchlorate
Formula Cl− ClO− ClO2− ClO3
− ClO4−
Structure
Polyatomic Cations are more rare
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Acetic Acid Dissolving in Water
+
Acetic Acid Water Acetate ion Hydronium ion