Chemical Bonding
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Transcript of Chemical Bonding
Chemical BondingChapter 13
Material on Midterm
How do 100 elements make up everything in the world?
Different types of bonds create differences in the properties of substances
From Glue to Goop
Objectives:◦Describe what chemical bonds are
◦Identify how many valence electrons are in any atom
◦Explain how you know if an atom is likely to form bonds
Section 1: Electrons and Chemical Bonding
Combining Atoms through Chemical Bonding◦Most atoms hate being alone…so they
bond!
Chemical bonding is the combining of atoms to form molecules or ionic compounds
Properties of new substance are different that the properties of the old substance
The chemical bond is the interaction that holds the two atoms together.
Section 1: Electrons and Chemical Bonding
6 + 6 + 12 =
C6H12O6
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Combining Atoms Through Chemical Bonding◦It’s all about the electrons
◦When bonds form, electrons can… …be shared …be gained …be lost
Section 1: Electrons and Chemical Bonding
Electron Number and Organization◦We need to organize the electrons so we
know what they will do if bonds are formed
Review: How do I know how many electrons at atom has?◦Same as its atomic number (proton #)
Section 1: Electrons and Chemical Bonding
What are the rules for where the electrons go?
Section 1: Electrons and Chemical Bonding
What are the rules for where electrons can go?◦Electrons do NOT like each
other! Will try to move FAR away from other electrons
ONLY pair up after 4 are on 2nd level◦N,S,E,W
Section 1: Electrons and Chemical Bonding
Outer-Level Electrons and Bonding◦Only the valence electrons are involved
in forming chemical bonds The valence electrons are the
electrons found in the outermost shell of an atom
Section 1: Electrons and Chemical Bonding
Section 1: Electrons and Chemical Bonding
Valence Electrons and the Periodic Table◦Elements in the same group have the
same number of valence electrons (generally)
◦If Lithium has 1…then Sodium, Potassium, rubidium, Cesium, and Francium all have…1!
Section 1: Electrons and Chemical Bonding
To Bond or Not to Bond◦Not all atoms bond the
same Group 18 have their
outmost shell filled.
WANNA GET TO 8! Group 18 already has 8
(except He), so they’re happy and DO NOT REACT
Section 1: Electrons and Chemical Bonding
To Bond or Not to Bond◦ Filling the Outermost Level
Less than 8? More likely to react. Will share, take, or lose electron(s) to get to the magic
number What about 2?
Some elements that are small (H, He, Li, Be), will try to get to 2 electrons for that first shell
Will share, take, or lose electron(s) to get to this number
Section 1: Electrons and Chemical Bonding
Section Review
1. Describe what chemical bonds are
2. Identify how many valence electrons are in any atom
3. Explain how you know if an atom is likely to form bonds
Section 1: Electrons and Chemical Bonding
Objectives:◦Explain how ionic bonds form◦Describe how positive and negative ions form
◦Explain why ionic compounds are neutral
Section 2: Ionic Bonds
Section 2: Ionic Bonds
All you need to know
about ionic bonding
is right here
Forming Ionic Bonds◦An ionic bond is a bond that forms when
electrons are transferred from one atom to another atom
◦This creates ions, which are charged particles that form when atoms gain or lose electrons
As a result of an ionic bond, either positive or negative ions can form
Section 2: Ionic Bonds
Forming Positive ions◦Positive ions form when metal atoms lost electrons
◦Na loses one electron---Na+
◦Ca loses two electrons –Ca2+
◦By losing electrons, metals can get to the magic number! Usually 8, could be 2
Section 2: Ionic Bonds
Forming Negative Ions◦Negative ions form when nonmetal atoms gain electrons
◦Cl gains one electron – Cl-◦O gains two electrons – O2-
◦By gaining electrons, nonmetals can get to the magic number! Usually 8, could be 2
Section 2: Ionic Bonds
Ionic Compounds◦When ionic bonds form, the number of electrons lost by the metal EQUALS the number of electrons gained by the nonmetals Everyone is happy!
◦The overall compound is neutral because the ions cancel out
Section 2: Ionic Bonds
When ions bond, they form a repeating 3D pattern called a crystal lattice◦Strong bonds mean: High melting points Brittleness High boiling points
Section 2: Ionic Bonds
Energy Energy is needed to lose an electron. ◦Very little energy is needed for Group I and II elements.
Energy is given off when atoms gain electrons. ◦Group 17 give off the most energy.
Section 2: Ionic Bonds
Section Review 1. Explain how ionic bonds form
2. Describe how positive ions form
3. Describe how negative ions form
4. Explain why ionic compounds are neutral
Section 2: Ionic Bonds
Objectives:◦Explain how covalent bonds form
◦Describe molecules◦Explain how metallic bonds form◦Describe the properties of metals
Section 3: Covalent and Metallic Bonds
What are Covalent Bonds◦A covalent bond forms when atoms
share one or more pairs of electrons
◦Occurs between nonmetals◦Helps them get to their MAGIC NUMBER
(8 or 2)
Section 3: Covalent and Metallic Bonds
Covalent Bonds and Molecules◦A molecule is the smallest unit of a substance that keeps all the physical and chemical properties of that substance 2 or more atoms joined in a definite ratio
Section 3: Covalent and Metallic Bonds
Covalent Bonds and Molecules◦ Easier way to draw them– Electron-Dot Diagrams
Remember, only the valence electrons are important for bonding!
Section 3: Covalent and Metallic Bonds
Covalent Bonds and Molecules◦To make an electron-dot diagram:
1. Write the symbol of the element in the center
2. Figure out how many valence electrons it has
3. Add valence electrons NSEW order4. You’re finished!
Section 3: Covalent and Metallic Bonds
Section 3: Covalent and Metallic Bonds Examples of electron-dot diagrams
• Models are useful for counting electrons in energy levels. But, these models do not show the true structure of an atom.
Atom v. molecule
Section 3: Covalent and Metallic Bonds
Atom Molecule
One type of element Two or more types of elements
Smallest particle into which an element can be divided and still be the same element
Smallest particle into which a covalently bonded compound can be divided and still be the same compound
Section 3: Covalent and Metallic Bonds
The Simplest Molecules◦ Must have at least two covalently bonded atoms
2 of the same element? Diatomic molecules Remember: HONClBrIF
Hydrogen Oxygen Nitrogen Chlorine Bromine Iodine Fluorine
Section 3: Covalent and Metallic Bonds
More Complex Molecules◦ Many different elements◦ Many based on carbon
Section 3: Covalent and Metallic Bonds
Metallic Bonds◦Metals have properties like malleability
and ductility because of their special bonds Metallic bonds are bonds from
between the attraction of positively charged metal ions and the electrons around them
Section 3: Covalent and Metallic Bonds
Movement of Electrons Throughout a Metal◦Bonding in metals is a result of the metal
atoms being so close to another that their outermost energy levels overlap
◦Metals surrounded in a “sea” of electrons
Section 3: Covalent and Metallic Bonds
Properties of Metals◦Conducting Electric Current Valence electrons that are moving
◦Reshaping Metals Electrons free to move around…makes it easy
to shape Ductility Malleability
◦Bending without breaking Electrons can move in response to pressure so
they can bend without breaking
Section 3: Covalent and Metallic Bonds
Alloys
Scientists can design alloys with specific properties by varying the types and amounts of elements in the alloy.
An alloy is a mixture of elements and at least one is a metal. Alloys have properties of metals.
Bronze = copper and tin
Steel = Iron and carbon
Airplanes = Aluminum and copper or manganese.
Section Review
1. Explain how covalent bonds form
2. Describe molecules
3. Explain how metallic bonds form
4. Describe the properties of metals
Section 3: Covalent and Metallic Bonds