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Questions and Answers
What is an ionic compound?
What is an ionic compound?
Crystalline solids with high melting points
What is a covalent bond?
What is a covalent bond?
Atoms held together by sharing electrons
What is a molecule?
What is a molecule?
Neutral group of atoms joined together by covalent bonds
What is a molecular compound?
What is a molecular compound?
What is a diatomic molecule?
What is a diatomic molecule?
Molecules of a given molecular compound are all the same.
Molecules of a given molecular compound are all the same.
How do ionic compounds exist?
How do ionic compounds exist?
What is the difference in boiling points between ionic and molecular (covalent) compounds?
What is the difference in boiling points between ionic and molecular (covalent) compounds?
What is the state of molecular compounds at room temperature?
What is the state of molecular compounds at room temperature?
What is a molecular formula?
What is a molecular formula?
Do molecular formulas tell you about a molecule's structure?
Do molecular formulas tell you about a molecule's structure?
What is the octet rule in covalent bonding?
What is the octet rule in covalent bonding?
What is a single covalent bond?
What is a single covalent bond?
What is an electron dot structure?
What is an electron dot structure?
What is a structural formula?
What is a structural formula?
What is a lone pair or unshared pair of electrons?
What is a lone pair or unshared pair of electrons?
Atoms form double or triple covalent bonds if they can attain a noble gas structure by sharing two or three pairs of electrons.
Atoms form double or triple covalent bonds if they can attain a noble gas structure by sharing two or three pairs of electrons.
What is a coordinate covalent bond?
What is a coordinate covalent bond?
What is a resonance structure?
What is a resonance structure?
What are exceptions to the Octet Rule?
What are exceptions to the Octet Rule?
What are molecular orbitals or orbital that apply to the entire molecule?
What are molecular orbitals or orbital that apply to the entire molecule?
What is a bonding orbital?
What is a bonding orbital?
What is a sigma bond?
What is a sigma bond?
What is a pi bond?
What is a pi bond?
What is VSEPR theory?
What is VSEPR theory?
What is a non-polar covalent bond?
What is a non-polar covalent bond?
What is a polar covalent bond?
What is a polar covalent bond?
What is a polar molecule?
What is a polar molecule?
When polar molecules are placed between oppositely charged plates, they become oriented with respect to the positive and negative plates.
When polar molecules are placed between oppositely charged plates, they become oriented with respect to the positive and negative plates.
Intermolecular attractions are weaker than either ionic or covalent bonds.
Intermolecular attractions are weaker than either ionic or covalent bonds.
What happens when you melt a network solid?
What happens when you melt a network solid?
What are intramolecular forces?
What are intramolecular forces?
What are intermolecular forces (IM)?
What are intermolecular forces (IM)?
What are London forces?
What are London forces?
What are dipole-dipole forces?
What are dipole-dipole forces?
What are hydrogen bonds?
What are hydrogen bonds?
Every bond is polar except diatomic.
Every bond is polar except diatomic.
What is bond dissociation energy?
What is bond dissociation energy?
How do double or triple covalent bonds form?
How do double or triple covalent bonds form?
How are oxygen atoms bonded in ozone?
How are oxygen atoms bonded in ozone?
How do electronegativity values determine the distribution of charge in a polar molecule?
How do electronegativity values determine the distribution of charge in a polar molecule?
Why do network solids have high melting points?
Why do network solids have high melting points?
When polar molecules are placed between oppositely charged metal plates, they tend to become oriented with respect to the positive and negative plates.
When polar molecules are placed between oppositely charged metal plates, they tend to become oriented with respect to the positive and negative plates.
What is bond length?
What is bond length?
Study Notes
Types of Compounds
- Ionic compounds: crystalline solids with high melting points, composed of positively and negatively charged ions arranged in repeating three-dimensional patterns
- Molecular compounds: composed of molecules, with lower melting and boiling points than ionic compounds
Bonds
- Covalent bond: atoms held together by sharing electrons
- Ionic bond: formed by the attraction between positively and negatively charged ions
- Single covalent bond: formed by sharing a pair of electrons
- Double covalent bond: formed by sharing two pairs of electrons
- Triple covalent bond: formed by sharing three pairs of electrons
Molecular Structure
- Molecule: neutral group of atoms joined together by covalent bonds
- Molecular formula: shows how many atoms of each element a molecule contains
- Electron dot structure: represents the shared pair of electrons of the covalent bond by two dots
- Structural formula: represents the covalent bonds by dashes and shows the arrangement of covalently bonded atoms
- Lone pair or unshared pair of electrons: a pair of valence electrons that is not shared between atoms
Octet Rule
- Octet rule: electron sharing occurs so that atoms attain the electron configuration of noble gases
- Exceptions to the octet rule: 1. odd number of valence electrons, 2. less than 8 electrons around the central atom, 3. more than 8 electrons around the central atom ("expanded octet")
Molecular Orbitals
- Molecular orbitals: when two atoms combine, their atomic orbitals overlap to produce molecular orbitals
- Bonding orbital: a molecular orbital that can be occupied by two electrons of a covalent bond
- Sigma bond: when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei
- Pi bond: when a pi molecular orbital is filled with two electrons
Intermolecular Forces
- Intermolecular forces: attractive forces that hold particles together, weaker than ionic or covalent bonds
- Van der Waals forces: weak forces that result from temporary shifts in the density of electrons in electron clouds
- London forces: weak forces that result from temporary shifts in the density of electrons in electron clouds, weakest type of intermolecular force
- Dipole-dipole forces: attraction between oppositely charged regions of polar molecules, stronger than London forces
- Hydrogen bonds: attraction between hydrogen and highly electronegative atoms (F, O, N)
Bond Dissociation Energy
- Bond dissociation energy: the amount of energy required to break a covalent bond
- Bond length: the distance between the nuclei of two bonded atoms
- Relationship between bond length and bond dissociation energy: the shorter the bond length, the higher the bond dissociation energy
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Description
This quiz covers types of compounds, bonds, and molecular structure in chemistry, including ionic and molecular compounds, covalent and ionic bonds, and molecular formulas.
