Term
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Definition
| protons + neutrons (nucleons) |
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Term
| What force holds p's and n's together in the nucleus of an atom? |
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Definition
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Term
| What are the differences in mass of e-'s, protons, and neutrons? |
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Definition
| protons and neutron about same (proton a little more), electron a lot less mass |
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Term
| the number of protons + neutrons in an atom is? |
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Definition
| The mass number, A, upper left hand of X |
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Term
| Think of an amu as about the mass od 1 proton or 1 neutron! |
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Definition
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Term
| In an isoelectric series: |
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Definition
- Is when the numer of electrons on each ion is the same
- Zeff will increase w/ increasing atomic number, Z, and draws electrons inwards w/ greater force
- Ion with fewest protons creates the weakest attrative force on the electrons and thus has the largest size
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Term
| The more negative ion will be greatest in size, so cations are larger than neutral and anions are smaller than neutral |
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Definition
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Term
| By definition, there are 12 amu in 1 atom of carbon-12 |
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Definition
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Term
Periodic Trends:
Energy of Ionization
Electron Affinity
Electronegativity |
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Definition
All increase from left to right ------> and from bottom to top
^
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Term
Periodic trends:
atomic radius
metallic character
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Definition
Increase from right to left <---------
and from top to bottom
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↓ |
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Term
Metals form: CATIONS
Nonmetals form: ANIONS
2 important aspects to KNOW about IONS:
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Definition
1. atoms lose electrons from highest energy shell 1st- in transition metals electrons are lost from s subshell 1st and then from d subshell
2. IOns are lookign fro symmetry- representative elemetns form noble gas configs when they make ions. transition metals try to even out their d orbitals so each orbital has the same number of electrons |
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Term
| Which elements exist as diatomic molecules? |
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Definition
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Term
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Definition
| A mole is the number of carbon atoms in 12 grams of C-12. |
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Term
| 1 gram= 6.022 * 10^23 amu |
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Definition
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Term
| moles= grams/ atomic or molecular weight |
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Definition
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