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Chemistry Ch. 8
Chemistry Test 8
| Question | Answer |
|---|---|
| What does a molecular formula tell us? | A molecular formula will tell you the types of elements and how many atoms present per molecule. |
| What are the types of models for a molecule? | -Molecular Formula. -Structural Formula. -Space-Filling. -Perspective. -Ball-and-Stick. |
| A single bond ends in... | -ane. |
| A double bond ends in... | -ene. |
| A triple bond ends in... | -yne. |
| Give the number and prefix for 1-5. | 1: Mono- 2: Di- 3: Tri- 4: Tetra- 5: Penta- |
| Give the number and prefix for 6-10. | 6: Hexa- 7: Hepta- 8: Octa- 9: Nona- 10: Deca- |
| ***Instead of one atom transferring electrons to anion(s), covalent bonds.... | Share electrons. |
| What is a coordinate covalent bond? | To help one atom, the other atom will donate more electrons. |
| Define a polyatomic ion. | Most contain both covalent and coordinate covalent bonds. Contains both covalent and ionic bonds. |
| What are the exceptions to the octet rule? | -Cannot be satisfied when the compound’s number of valence electrons is an odd number Nitrogen dioxide Chlorite and nitrogen monoxide -Even number: Boron with fluorine. |
| What are Bond Dissociation Energies? | -Energy required to break the bonds between two covalently bonded atoms. -Measured in kJ/mol. -More energy= stronger bond. |
| Define Resonance Structures. | Used to show the bonding that cannot adequately be shown with a single structure -Double headed arrows are used to connect resonance structures. |
| What's the difference between molecular orbitals and covalent bonds? | Molecular orbitals- Belongs to a molecule as a whole Covalent bond- Bonding orbital. |
| What is a sigma bond? | Symmetrical around the axis connecting two atomic nuclei. |
| What are pi bonds? | Side-by-side overlap of atomic p-orbitals (sausage shaped regions above and below axis). |
| What is molecular polarity? | The uneven distribution of molecular charge. |
| What determines molecular polarity? | The polarity of each bond, along with the geometry of the molecule. |
| What are the two parts of molecular polarity (definitions)? | Molecule: -Atoms held together by a bond Polarity: -Uneven distribution of charge. |
| What does the VSEPR Theory do? | Helps predict the geometries (shape) of more-complicated molecules by Considering all the locations of all electron pairs surrounding the bonded atoms. |
| What is the VSEPR Theory? | States that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible. -The shared electrons are oriented as far away from each other as possible. |
| What is ABE? | We represent the central atom with the letter A, atoms bonded to the central atom with the letter B, and the lone-pair electrons with the letter E. |
| What is hybridization? | The mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies. |
| Define hybrid orbitals. | Orbitals of equal energies produced by the combination of two or more orbitals on the same atom |
| Define intermolecular force. | The forces of attraction between molecules. |
| Define molecular polarity. | Polar molecules act as tiny dipoles because of their uneven charge distribution. |
| Define dipole. | Is created by equal but opposite charges that are separated by a short distance. |
| Define dipole-dipole. | Forces of attraction between polar molecules. |
| Define Hydrogen bonding. | A hydrogen atom is bonded to a highly electronegative atom. Particularly strong type of dipole-dipole force, explains the unusually high boiling points of some hydrogen-containing compounds |
| Define London Dispersion Forces. | Resulting from the constant motion of electron and the creation of instantaneous dipoles. |
| How are dipole's represented? | By an arrow with a head pointing toward the negative pole and a crossed tail situated at the positive pole. |
| How are dipole molecules? Far? Close? | Forces are short-range forces, acting only between nearby molecules. |
| _______ _______ is a special case of dipole-dipole forces. | Hydrogen Bonding. |
| For molecules containing more than two atoms, molecular polarity depends on... | Both the polarity and the orientation of each bond. |
| What makes Hydrogen Bonds make the connection highly polar? | The large electronegativity differences between hydrogen atoms and fluorine, oxygen, or nitrogen. |
| What is Hydrogen Bonding represented by? | Usually representing by dotted lines connecting the hydrogen-bonded hydrogen to the unshared electron pair of the electronegative atom |
| Go into detail about London Dispersion Forces. | Electrons are in continuous motion, creating an instantaneous uneven distribution. Create a positive pole on one part and a negative pole on the other side. The temporary dipole can induce a dipole in an adjacent atom. |
| Network solids are very... | Stable. |
Created by:
OliviaRoark
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