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Questions and Answers
What are the two ways atoms acquire completed valence shells?
What are the two ways atoms acquire completed valence shells?
Ionic bond and covalent bond
What happens to electrons in an ionic bond?
What happens to electrons in an ionic bond?
Electrons are completely transferred from one atom to another of a different element
What is the name given to the charged particles formed in an ionic bond?
What is the name given to the charged particles formed in an ionic bond?
Ions
How do atoms interact in a covalent bond?
How do atoms interact in a covalent bond?
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Which of these is NOT a type of hybrid orbital?
Which of these is NOT a type of hybrid orbital?
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The combination of two or more atomic orbitals forms a new set of atomic orbitals called hybrid orbitals. This process is called hybridization.
The combination of two or more atomic orbitals forms a new set of atomic orbitals called hybrid orbitals. This process is called hybridization.
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What type of hybrid orbital is formed by combining one s orbital and three p orbitals?
What type of hybrid orbital is formed by combining one s orbital and three p orbitals?
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What is the shape of a molecule with sp3 hybridization?
What is the shape of a molecule with sp3 hybridization?
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What geometry do molecules that are sp2 hybridized have?
What geometry do molecules that are sp2 hybridized have?
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What kind of geometry do molecules with sp hybridization have?
What kind of geometry do molecules with sp hybridization have?
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Study Notes
Chemical Bonding
- Atoms interact to achieve a completed outer electron shell configuration, resembling a nearby noble gas.
- Atoms achieve complete valence shells via two types of bonds: ionic and covalent.
Ionic Bond
- Electrons are completely transferred from one atom to another.
- This creates charged particles called ions.
- A chemical bond formed by electron transfer is called an ionic bond.
- Examples include Sodium (Na) and Chlorine (Cl), forming Sodium Chloride (NaCl).
- Sodium loses an electron, becoming positively charged (Na+) and Chlorine gains an electron, becoming negatively charged (Cl-).
- In the resulting crystal lattice, oppositely charged ions attract.
Covalent Bond
- Atoms share electrons to complete their valence shells.
- A chemical bond formed by sharing electrons is called a covalent bond.
- Covalent bonds can be polar or nonpolar, influenced by the electronegativities of the atoms involved.
- A larger difference in electronegativity leads to a more polar bond.
- Example: two chlorine atoms sharing electrons to form a Cl2 molecule.
Coordinate Bond
- A bonding mechanism where one atom provides both electrons shared in the bond.
Hybridization
- This refers to the mixing of atomic orbitals to form new, hybrid orbitals, explaining observed bond angles in molecules.
- The premise is that simple atomic orbitals don't fully explain molecular structures' angles.
Hybridization of Orbitals
- Combining atomic orbitals to form new ones (hybrid orbitals) is the process of hybridization.
- This adjustment explains observed bond angles that are not solely 90°.
- These new hybrid orbitals offer better explanations of molecular shape and bonding.
Types of Hybridization
- sp3: One 's' orbital combines with three 'p' orbitals.
- sp2: One 's' orbital combines with two 'p' orbitals.
- sp: One 's' orbital combines with one 'p' orbital.
Types of Chemical Bonds / Types of Covalent Bonds
- Polar covalent bond, when the difference of electronegativity is considerable between two atoms and electrons are shared unequally creating partial charges in a molecule.
- Non-polar covalent bond, when the difference of electronegativity is negligible between two atoms and electrons are shared equally in a molecule.
Formation of Chemical Bond
- Overlapping hybrid orbitals result in different types of bonds depending on the overlap geometry.
- "Direct" overlap forms sigma (σ) bonds.
- "Parallel" overlap forms pi (π) bonds.
Examples of Hybridization
- Methane (CH4) exhibits sp3 hybridization.
- Ethane (C2H6) exhibits sp3 hybridization.
- Ethylene (C2H4) exhibits sp2 hybridization.
- Formaldehyde exhibits sp2 hybridization.
- Acetylene (C2H2) exhibits sp hybridization.
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Description
Explore the foundational concepts of chemical bonding, including ionic and covalent bonds. Learn how atoms interact to form stable configurations through electron transfer and sharing. This quiz covers the essential principles essential for understanding chemistry.
