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Questions and Answers
What does a higher electronegativity indicate about an atom's ability?
What does a higher electronegativity indicate about an atom's ability?
- It can attract a bonding pair of electrons more strongly. (correct)
- It completely lacks the ability to form bonds.
- It has a higher tendency to repel bonding electrons.
- It has a lower attraction force for bonding electrons.
Which of the following bonds is classified as polar covalent?
Which of the following bonds is classified as polar covalent?
- Bonds with a difference in electronegativity of 2.1 and more
- Bonds with a difference in electronegativity of 0.4 – 1
- Bonds with a difference in electronegativity of 1 – 2.1 (correct)
- Bonds with a difference in electronegativity of 0 – 0.4
In a non-polar covalent bond, how do the atoms interact with shared electrons?
In a non-polar covalent bond, how do the atoms interact with shared electrons?
- One atom attracts the shared electrons more than the other.
- Shared electrons are completely transferred to one atom.
- Shared electrons are only partially attracted to one atom.
- Both atoms attract the shared electrons equally. (correct)
What condition does NOT lead to a polar molecule, even if a polar bond exists?
What condition does NOT lead to a polar molecule, even if a polar bond exists?
When analyzing molecular polarity, which situation indicates a polar molecule?
When analyzing molecular polarity, which situation indicates a polar molecule?
What does electronegativity measure in an atom?
What does electronegativity measure in an atom?
Which electronegativity difference indicates a non-polar covalent bond?
Which electronegativity difference indicates a non-polar covalent bond?
In a polar covalent bond, what happens to the charges of the atoms involved?
In a polar covalent bond, what happens to the charges of the atoms involved?
What electronegativity difference is classified as ionic?
What electronegativity difference is classified as ionic?
Which of the following statements about polar bonds is true?
Which of the following statements about polar bonds is true?
What is a characteristic of a non-polar molecule?
What is a characteristic of a non-polar molecule?
Which of these examples represents a polar molecule?
Which of these examples represents a polar molecule?
How can you determine if a molecule with polar bonds is polar?
How can you determine if a molecule with polar bonds is polar?
What usually happens in a polar covalent bond?
What usually happens in a polar covalent bond?
Which of these statements is NOT true about electronegativity?
Which of these statements is NOT true about electronegativity?
Study Notes
Electronegativity
- A measure of an atom's tendency to attract bonding electrons.
- Higher electronegativity means stronger attraction for bonding electrons.
- Represented by decimal numbers on the periodic table, next to each element.
Bonds and Electronegativity Difference
- Non-polar covalent bond: Electronegativity difference (∆EN) is between 0 and 0.4.
- Covalent and very weak polar covalent bond: ∆EN is between 0.4 and 1.
- Polar covalent bond: ∆EN is between 1 and 2.1.
- Ionic bond: ∆EN is 2.1 or greater.
Non-polar vs. Polar Covalent Bonds
- Non-polar: Atoms equally attract shared electrons.
- Polar: One atom attracts shared electrons more strongly than the other.
- This leads to a slightly negative charge on the stronger attracting atom and a slightly positive charge on the other.
- A polar bond doesn't automatically mean a polar molecule.
Checking for Polarity
- Draw the shape of the molecule.
- Determine the polarity between atoms.
- Check the positions of δ+ and δ- :
- If both δ+ and δ- are outside the molecule's shape, it is polar.
- If δ+ or δ- is only on the outside, it is non-polar.
- Important: Polar bonds don't always result in polar molecules.
Examples of Molecules
- Two atoms: HCl, F2, HBr
- Three atoms: H2O, CO2
- Four atoms: BF3, NH3
- Five atoms: CCl4, CH3Cl
Electronegativity
- A measure of an atom's tendency to attract shared electrons in a bond.
- Higher electronegativity indicates stronger attraction to bonding electrons.
- Represented by a decimal number associated with each element on the periodic table.
Bond Types and Electronegativity Differences
- Non-polar Covalent: Electronegativity difference (ΔEN) between 0 and 0.4. Atoms share electrons equally.
- Covalent and Very Weak Polar: ΔEN between 0.4 and 1. Electrons are shared unequally, but the difference is small.
- Polar Covalent: ΔEN between 1 and 2.1. One atom attracts electrons more strongly, creating partial positive and negative charges.
- Ionic: ΔEN greater than 2.1. One atom completely gains electrons, forming a positive ion, while the other forms a negative ion.
Determining Polarity
- Non-polar Covalent: Both atoms attract electrons equally.
- Polar Covalent: One atom attracts electrons more strongly, creating a slightly negative charge (δ-) around that atom and a slightly positive charge (δ+) around the other atom.
- Polar Molecule: The overall molecule has a positive and negative end due to uneven distribution of electron density.
- Non-polar Molecule: The molecule has an even distribution of charge, even with polar bonds.
Examples of Molecules
- Two Atoms: HCl, F2, HBr
- Three Atoms: H2O, CO2
- Four Atoms: BF3, NH3
- Five Atoms: CCl4, CH3Cl
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Description
Test your knowledge on electronegativity and the types of chemical bonds. This quiz covers concepts from non-polar to polar covalent bonds and ionic bonds, along with how to determine molecular polarity. Perfect for chemistry students looking to strengthen their understanding of bonding concepts.
