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freshmanchemexam1/2
first and second exam of freshman chem
| Question | Answer |
|---|---|
| Aufban Principle | as you add protons to the nucleus as you go through the periodic table, you add electrons to atomic orbitals |
| which elements have weird e- configurations? what's different about them? | Cr and Cu (as well as first row of transition metals other than cobalt) - fill up d shell to 5 or 10 instead of filling up 4s shell |
| unpaired e- = | paramagnetic |
| all paired e- = | diamagnetic |
| column 1 of periodic table | Alkali Metals |
| Column 2 of periodic table | Alkaline earth metals |
| Column 17 of periodic table | halogens |
| Column 18 of periodic table | noble gases |
| representative elements | "main group", not transition metals |
| e- configuration for representative cations | remove e- from highest n shell |
| e- configuration for representative anions | add e- to highest partially filled n shell |
| isoelectronic | have same number of e- |
| e- configurations for transition metals | remove the 4s e- first, and then the 3d |
| Effective Nuclear Charge = | atomic size and the ability to lose e- (ionization) |
| Effective nuclear charge increases.... | Left to right on a periodic table |
| ionic radius = | radius of cation/anion |
| for anions, what's bigger? original or anion? | anion (added electron) |
| for cations, what's bigger? original or cation? | original (lost electron) |
| ionization energy = | energy needed to remove e- from a gaseous atom/ion. measures how tightly e- are held |
| the ____ the ionization energy, the harder it is to remove e- | bigger |
| what has a higher ionization energy, metals or nonmetals? | nonmetals |
| electronegativity increases... | bottom to top and left to right on periodic table |
| the more ___ electron affinity, the more likely it is to gain an e- | positive |
| a stable anion's electron affinity is | large and positive |
| halogens electron affinity are | high and positive |
| atoms achieve maximum stability when.... | isoelectronic w/ a noble gas |
| covalent bonds = | sharing e- between 2 atoms follows octet rule |
| electronegativity = | unequal sharing of e- |
| formal charge is calculated as... | the difference between # of valence e- in atom, and # of e- atom has in lewis structure. |
| formal charge should ideally be | as equal as possible to zero if atom is neutral, and equal to the charge if atom has one. |
| exceptions to the octet rule | incomplete octet, odd number of e-, expanded octet |
| which elements can have an incomplete octet? | Be and B |
| what kind of combinations of elements have an odd number of e-? | radicals |
| which elements can have expanded octets? | 3rd row and beyond |
| electronegativity (in a bond) is? | the ability of an atom to pull e- towards itself in a covalent bond |
| number of protons in an atom = | atomic number |
| number of neutrons in an atom = | mass number - number of protons |
| number of electrons in an (neutral) atom = | same as number of protons |
| number of electrons in a charged atom = | number of protons +/- charge |
| principal quantum number = | (n) describes the size of the orbital |
| angular quantum number = | (l) describes the shape of the orbital |
| Orbitals have shapes that are best described as spherical have an l of | 0 |
| Orbitals have shapes that are best described as polar have an l of | 1 |
| Orbitals have shapes that are best described as cloverleaf have an l of | 2 |
| magnetic quantum number = | (ml) describes the orientation in space of a particular orbital. |
| for the 5f subshell, the n = | 5 |
| for a 3d subshell, the n = | 3 |
| possible values of l | 0 to n-1 |
| l value for the s orbital | 0 |
| l value for the p orbital | 1 |
| l value for the d orbital | 2 |
| l value for the f orbital | 3 |
| possible values for ml | -l to +l |
| ionic radius increases | right to left top to bottom |
| atomic radius increases | right to left top to bottom |
| electron affinity increases | left to right bottom to top |
| ionization energy increases | left to right bottom to top |
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