Term
| JJ Thompson's cathode ray tube determined |
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Definition
| electrons existed in atoms |
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Term
| the gold foil experiment determined |
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Definition
| that protons existed in atoms |
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Term
| An experiment performed by Robert ----- in 1909 determined the size of the charge on an electron |
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Definition
|
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Term
|
Definition
A-mass number
Z-atomic number
X-element symbol |
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Term
Periodic table mass is the
weighted ----
of all of
the isotopes of each element |
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Definition
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Term
| according to the electromagnetic spectrum, visible light ranges from _____ (left end) to ____ (right end). What are the respective wavelengths of these two extremas? |
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Definition
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Term
| produced by oscillating motion of electric charge |
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Definition
|
|
Term
According to the Photoelectric effect and theory, quantity of e–
depends on
---- of light |
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Definition
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Term
| According to the Photoelectric effect and theory, photons are only ejected if |
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Definition
| light shined at or above minimum frequency on metal surface |
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Term
| T/F: the atomic line spectrum is continuous |
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Definition
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Term
| as electrons absorb energy, they move to a ______, also known as the excited state |
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Definition
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Term
| as electrons fall back to a lower orbital, ____ is released as _____ |
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Definition
| light is released as energy |
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Term
|
Definition
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|
Term
|
Definition
|
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Term
| For sig figs and problems that involve multiple calculations with only division or multiplication... |
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Definition
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|
Term
| For sig figs and problems that involve multiple calculations with addition/subtraction AND multiplication/division... |
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Definition
| sig figs are defined at EACH step |
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Term
|
Definition
|
|
Term
| the principle quantum number (n) is proportional to |
|
Definition
the average distance
of the e-
from the nucleus |
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|
Term
| Angular Momentum Quantum Number (l) describes |
|
Definition
|
|
Term
| what letters corresponds to each of the principle quantum numbers: 0, 1, 2, 3 |
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Definition
|
|
Term
| Magnetic Quantum Number (ml) |
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Definition
| describes orientation of the orbital |
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Term
| • All orbitals in a subshell have --- energy |
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Definition
|
|
Term
| Electron Spin Quantum Number (ms) |
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Definition
|
|
Term
| Pauli Exclusion Principle states that |
|
Definition
Each orbital can only have 2 e-
e- in same orbital have opposite spin |
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|
Term
in
1s2 2s2 2p6 3s2 3p3 electron configuration of phosphorus, which are the core electrons vs valence electrons |
|
Definition
core: 1s2 2s2 2p6
valence: 3s2 3p3 |
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Term
| special cases in which the electron configuration of certain elements (in the d-orbital range) do not follow the trend arises from what fact regarding d-orbitals? |
|
Definition
| ½ filled or completely filled d orbital is more stable |
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Term
|
Definition
| electrons fill from lowest to highest energy |
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|
Term
|
Definition
| most stable orbital is where you try to get all orbitals to have same e- spin |
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Term
| to find the debroglie wavelength... |
|
Definition
| divide planck's constant by the product of mass and velocity |
|
|
Term
| the element P has the ions P- and P+, place them in order of smallest ionic radius to largest |
|
Definition
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|
Term
Amount of energy required to completely convert
one mole of a solid ionic compound to the
constituent ions in the gas phase |
|
Definition
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|
Term
| ____ bonding Gives each atom a noble gas configuration |
|
Definition
|
|
Term
| what is the difference between pure covalent and polar covalent? ionic? |
|
Definition
pure- electrons are equally shared
polar- unequally shared
ionic- opposite charges |
|
|
Term
ability of an atom in a
compound to attract electrons to itself |
|
Definition
|
|
Term
List the type of bonding that occurs in the respective electronegativity differences
<0.5
0.52.0
>2.0 |
|
Definition
nonpolar covalent
polar covalent
ionic |
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Term
| when drawing lewis structures, we have to consider that ____(element) only forms two bonds and _____(element) can only form 3 |
|
Definition
|
|
Term
| three rules of naming covalent compounds |
|
Definition
1 add prefixes for both element
2 drop mono for first element
3 add -ide suffice to second element |
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|
Term
| three rules of naming ionic compounds whose cation has 1 charge |
|
Definition
1 write metal
2 add -ide if monoatomic anion
3 write name for polyatomic anion |
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|
Term
| four rules of naming ionic compounds whose cation has multiple charges |
|
Definition
1 write metal
2 specify charge with roman numerals
3 add -ide if monoatomic anion
4 write name for polyatomic anion |
|
|
Term
| go over common polyatomic ion names |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
anion ends in -ate, add -ic
anion ends in -ite, add -ous |
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|
Term
what molecules have a SPECIFIC number of
waters in their structure?
what indicates the number of water molecules in the compound |
|
Definition
|
|
Term
| what type of acid has only one hydrogen |
|
Definition
binary acids
e.g. hydrochloric acid HCL |
|
|
Term
Contain carbon and
hydrogen |
|
Definition
|
|
Term
| Covalently bonded to form a single ion |
|
Definition
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|
Term
| Metals lose electrons from the ____ shell |
|
Definition
|
|
Term
| how to determine the polarity of a molecule? Check what two things? |
|
Definition
| lone pairs and polar bonds. what are polar bonds? |
|
|
Term
| In VB theory, a single bond is represented by |
|
Definition
|
|
Term
| In VB theory, a double bond is represented by |
|
Definition
| 1 sigma bond and 1 pi bond |
|
|
Term
| In VB theory, a triple bond is represented by |
|
Definition
| 1 sigma bond and 2 pi bonds |
|
|
Term
Carbon always
has a complete
octet (put in
---
where
necessary) |
|
Definition
|
|
Term
| In organic molecules, what element symbol is usually not written? |
|
Definition
| carbon/ Carbon-Hydrogen bond |
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|
Term
|
Definition
|
|
Term
| Draw sulfite ion, what should you take into consideration? How many resonance structures does it have? |
|
Definition
|
|
Term
| To find ideal bond angles, look at electron domain geometry chart or molecular geometry chart? |
|
Definition
| based on electron domain geometry |
|
|
Term
|
Definition
|
|
Term
_________________________________________________
24. What is the name of the compound formed when HI is dissolved in water? |
|
Definition
|
|
Term
_____________________________________________________
27. Resonance structures differ by: |
|
Definition
| . placement of electrons only |
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|
