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Questions and Answers
What type of bonding occurs when two or more non-metals share a pair of electrons?
What type of bonding occurs when two or more non-metals share a pair of electrons?
In VSEPR theory, which shape corresponds to a central atom with four bonded pairs and no lone pairs?
In VSEPR theory, which shape corresponds to a central atom with four bonded pairs and no lone pairs?
Which statement about electronegativity is true?
Which statement about electronegativity is true?
Which type of molecule is likely to be soluble in a non-polar solvent?
Which type of molecule is likely to be soluble in a non-polar solvent?
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What are the two types of intermolecular forces that can keep molecules together?
What are the two types of intermolecular forces that can keep molecules together?
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Which of the following statements about hydrogen bonding is true?
Which of the following statements about hydrogen bonding is true?
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Which of the following interactions is characterized by the presence of a net pull due to uneven electron sharing?
Which of the following interactions is characterized by the presence of a net pull due to uneven electron sharing?
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What is the relationship between the strength of intermolecular forces and boiling points?
What is the relationship between the strength of intermolecular forces and boiling points?
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Study Notes
Ionic Bonding
- Atoms tend to obey the octet rule.
- Held together by ionic (or electrovalent) bonds.
- Many ions form a lattice structure.
- Ionic bonds involve a transfer of electrons.
Covalent Bonding
- Involves sharing electrons.
- Formed between two or more nonmetals.
- Covalent bonds create molecular compounds.
- The central atom is usually the atom with the most bonding electrons.
- Carbon is the central atom 99% of the time.
VSEPR Theory
- Valance Shell Electron Pair Repulsion Theory.
- Predicts the basic shapes around central atoms (linear, angular, trigonal, tetrahedral, trigonal planar).
- The placement of secondary elements influences shape.
- Dashed lines represent bonds behind the plane, wedges represent bonds in front of the plane.
Electronegativity
- Electronegativity is a measure of an atom's ability to attract electrons in a covalent bond.
- Higher electronegativity means greater pull on electrons.
- Electronegativity values are found on the periodic table.
- If two atoms have the same electronegativity, the bond is polar, no element has a stronger pull..
Polar/Nonpolar Covalent Bonds
- Nonpolar: Electrons shared equally. No net pull on electrons, meaning it cancels out.
- Polar: Electrons shared unequally. There's a net pull on one atom.
Polar Molecules
- Electrons shared unequally.
- Polar molecules will have a net pull (not canceled out).
- Group 15 elements are always polar.
- Solubility: "Like dissolves like". Polar solids dissolve in polar solvents, nonpolar solids dissolve in nonpolar solvents.
Intermolecular Forces in Molecular Compounds
- Intramolecular forces: Hold atoms within a molecule together.
- Intermolecular forces: Hold molecules together.
- Two main types of intermolecular forces are Van Der Waals forces and hydrogen bonding.
London Dispersion Forces
- The strength of London dispersion forces is related to the energy needed to separate molecules and to boiling point.
- The greater the force, the higher the boiling point.
Dipole-Dipole Forces
- Dipole-dipole forces require polar molecules.
Hydrogen Bonding
- Hydrogen bonding occurs when hydrogen is bonded to a highly electronegative atom (F, O, or N).
- A hydrogen bond is an intermolecular force that occurs when a hydrogen atom covalently bound to a very electronegative atom is attracted to another electronegative atom in a nearby molecule also.
- Molecules with stronger intermolecular forces (IMFs) have higher boiling points.
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Description
Test your understanding of ionic and covalent bonding concepts, including the octet rule, electron transfer, and electron sharing. Dive into VSEPR theory to predict molecular shapes and explore electronegativity's role in bond formation. This quiz covers essential topics in chemistry.
