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Questions and Answers
What type of bond is formed when electrons are unequally shared between two atoms?
What type of bond is formed when electrons are unequally shared between two atoms?
- Metallic bond
- Polar covalent bond (correct)
- Pure covalent bond
- Ionic bond
Electronegativity increases as you move down a group on the periodic table.
Electronegativity increases as you move down a group on the periodic table.
False (B)
What does a dipole moment measure?
What does a dipole moment measure?
The polarity of a molecule
In a water molecule, oxygen has a partial ______ charge.
In a water molecule, oxygen has a partial ______ charge.
If the electronegativity difference between two atoms is 0, what type of bond is likely to form?
If the electronegativity difference between two atoms is 0, what type of bond is likely to form?
The atomic radius increases as you move across a period on the periodic table.
The atomic radius increases as you move across a period on the periodic table.
What is the molecular geometry of a water molecule?
What is the molecular geometry of a water molecule?
Match the following bond types with their descriptions:
Match the following bond types with their descriptions:
A molecule with only non-polar covalent bonds will always be a polar molecule.
A molecule with only non-polar covalent bonds will always be a polar molecule.
What causes the unique properties of water, such as its high boiling point?
What causes the unique properties of water, such as its high boiling point?
What two criteria must be met for a molecule to be considered polar?
What two criteria must be met for a molecule to be considered polar?
The electron geometry describes the arrangement of all electron areas around a central atom, including bonding and ______ pairs.
The electron geometry describes the arrangement of all electron areas around a central atom, including bonding and ______ pairs.
Match the following molecular shapes with their descriptions:
Match the following molecular shapes with their descriptions:
According to the rules, which of these molecules is non-polar?
According to the rules, which of these molecules is non-polar?
The carbon-oxygen bond in carbon dioxide is considered non-polar.
The carbon-oxygen bond in carbon dioxide is considered non-polar.
What causes the opposing dipoles in carbon dioxide to cancel out, making the molecule non-polar?
What causes the opposing dipoles in carbon dioxide to cancel out, making the molecule non-polar?
Flashcards
Electron Geometry
Electron Geometry
The arrangement of all electron pairs around a central atom, including both bonding and lone pairs
Molecular Geometry
Molecular Geometry
The arrangement of only the bonding electron pairs around a central atom.
Bent Molecular Shape
Bent Molecular Shape
A molecule with a non-linear shape, meaning the atoms are not all aligned in a straight line.
Polar Molecule
Polar Molecule
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Non-polar Molecule
Non-polar Molecule
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ΔEN
ΔEN
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Diatomic Molecule
Diatomic Molecule
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Polyatomic Molecule
Polyatomic Molecule
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Electronegativity
Electronegativity
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Pure Covalent Bond (Non-Polar Covalent)
Pure Covalent Bond (Non-Polar Covalent)
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Polar Covalent Bond
Polar Covalent Bond
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Electronegativity Difference
Electronegativity Difference
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Dipole Moment
Dipole Moment
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Electron Arrangement
Electron Arrangement
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Molecular Shape
Molecular Shape
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Ionic Bond
Ionic Bond
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Study Notes
Determining Bond and Molecular Polarity
- Electronegativity (EN) is a measure of an atom's ability to attract shared electrons in a chemical bond.
- Ionic bonds involve the transfer of electrons between a metal and non-metal. Electronegativity difference is greater than 1.7. Example: NaCl.
- Polar covalent bonds involve unequal sharing of electrons between two nonmetals. Electronegativity difference is between 0.4 and 1.7. Example: Hâ‚‚O.
- Pure (non-polar) covalent bonds involve equal sharing of electrons between two nonmetals. Electronegativity difference is 0. Example: Oâ‚‚.
Electronegativity Trends
- Electronegativity generally increases across a period (left to right) on the periodic table.
- Electronegativity generally decreases down a group (top to bottom).
- Fluorine (F) is the most electronegative element.
- Francium (Fr) is the least electronegative element.
Polar Covalent Bonds
- A polar covalent bond is formed when the bonding pair of electrons is unequally shared between two atoms because one atom has a stronger affinity for electrons.
- The atom with the stronger electron affinity develops a partial negative charge (δ–).
- The other atom develops a partial positive charge (δ+).
- Example: In a hydrogen chloride (HCl) molecule, chlorine is more electronegative than hydrogen, attracting the shared electrons more strongly resulting in a δ– charge on chlorine and a δ+ charge on hydrogen.
Molecular Shapes and Polarity
- The arrangement of atoms in a molecule, its molecular shape, determines if the molecule is polar or nonpolar.
- If a molecule contains polar bonds but it is symmetrical, the polar bonds cancel each other out, and the molecule is nonpolar. Example: Carbon dioxide (COâ‚‚).
- If a molecule contains polar bonds and it is asymmetrical, the molecule is polar. Example: Water (Hâ‚‚O).
- Molecules with lone pairs around the central atom can also influence the molecular polarity, even with symmetrical arrangements of bonds.
- Different molecular shapes result from the need to maximize the distances between electrons in a molecule.
Determining Molecular Polarity
- A molecule is polar if it:
- Contains polar bonds
- Is asymmetrical in shape, and/or contains lone pairs.
- In summary: Polar molecules have a positive and a negative end.
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Description
This quiz assesses your understanding of electronegativity, bond types, and molecular polarity. You'll explore topics such as ionic bonds, polar covalent bonds, and the trends in electronegativity across the periodic table. Test your mastery of these essential chemistry concepts!
