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chemistry ch 6 test
Chemistry chapter 6 test
| Question | Answer |
|---|---|
| a force that holds two atoms together | chemical bond |
| a bond formed by sharing valence electrons | covalent bond |
| a neutral group of atoms that are held together by covalent bonds | molecule |
| bonding when electrons are shared equally resulting in balanced distribution of charge | nonpolar covalent bonds |
| bonded atoms that have an unequal attraction for the shared electrons | polar |
| chemical compound whose simplest units are molecules | molecular compound |
| indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts | chemical formula |
| shows the types and numbers of atoms combined in a single molecule of a molecular compound | molecular formula |
| a molecule with only 2 atoms | diatomic molecule |
| the distance between two bottom atoms at their minimum potential energy (the average distance between two bonded atoms) | bond length |
| shorter the bond length = __________ | the stronger the bond |
| energy required to break a chemical bond | bond energy |
| chemical compounds tend to form so that each atom has an octet of electrons in its highest occupied energy level (or in other words elements want 8 electrons) | octet rule |
| exceptions to the octet rule: | hydrogen and helium - only needs 2 Boron - (i have both 3 and 6 as answers so im not sure which is right) |
| Lewis dot structure is where we do all that stuff with the dots | |
| when a single pair of electrons is shared Ex: H-H | single covalent bonds |
| there can be two single covalent bonds Ex: H-O-H (makes H20) since oxygen has 6 electrons it needs 2 more to make it happy so it makes single bonds with hydrogen | |
| there can be three single covalent bonds Ex: NH3 (if you dont understand this one it is on slide 23) | |
| there can be four single covalent bonds Ex:CH4 | |
| read about the lewis dot structure slides 25-28 | |
| if you have an unshared pair that is not involved in bonding | lone pairs |
| sharing more than one pair of electrons between two atoms | multiple covalent bonds |
| example of multiple bonds: Oxygen can form a double bond because one oxygen has 6 electrons Nitrogen can form a triple bond because if has 5 electrons | |
| as you increase from a single bond to a triple bond, the bond length _____ | decreases |
| look at resonance structures on slide 35 and 36 (hard to put on a slide) | |
| chemical bonding that results form the electrical attraction between large numbers of cations and anions | ionic bonding |
| compounds that contain ionic bonds | ionic compounds |
| an ion formed from only one atom | monatomic ion |
| ions made up of more than one atom | polyatomic ions |
| uneven distribution of molecular charge | molecular polarity |
| repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible | VSEPR theory |
| VSEPR stands for: | Valence Shell Electron Pair Repulsion |
| angle formed by an two terminal atoms and the central atom | bond angle |
| a process in which atomic orbital's are mixed to form new, identical hybrid orbitals | hybridization |
| forces of attraction between molecules | intermolecular forces |
| examples of intermolecular forces: | dipole-dipole - only polar london dispersion - weakest hydrogen bonding - strongest |
Created by:
natalie.hardy