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AP Chemistry None with None at Syracuse University

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By: Gerri Blick
Created: 2011-05-21
Size: 42 flashcards
Views: 27

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energy of electrons in further vs. closer orbitals

the further from the nucleus the higher the energy, closer to the nucleus the energy goes down--electrons closer to the nucleus have less energy because thats where they want to be since electrons are negative and overall charge of nucleus is positive due to protons.

mass number

designates a specific isotope

protons + neutrons

²³⁵U-- the upper number

atomic number

defines what element we are talking about

tells the number of protons

₉₂U-the lower number

what happens if you change the number of electrons in an atom

gives the atom a charge and makes it an ion

what happens if you change the neutrons in an atom

makes it a different isotope of that same atom and gives it a different mass number

what happens if you change the protons of an atom

makes it a different element

basics of periodic table

columb=group-up and down

row=period -left ot right

noble gas=inert-no chemical reactions involved

alkali metal (group 1)-basic, highly reactive in water and as you go down they become more reactive

alkaline earth metal (group 2)-create basic solutions but less reactive than group 1

transition metals-take on various charges

halogens-group 7-have 7 valence electrons want to pick up one more.

how many electrons are held in each shell?

2n²

degenerate

when orbitals are equal in energy

ex: p orbital has 3 degenerate orbitals

how can you get a more stable shell?

half filled subshells and completely filled subshells are more stable than 1 away from being full.

electron configuration of Cu

EXCEPTION!

Cu would think to be [Ar]4s²3d⁹

but its actualy [ar] 4s¹3d¹⁰

ag and au and rg also follow this exception.

electron configuration for Cr and Mo

Exceptions!

Cr: [Ar] 4s¹3d⁵

Mo: [Kr] 5s¹4d⁵

this is NOT an exception for W and Sg

electron configuration for Cu²⁺

move from highest shell number first, so 4 before 3.

Cu²⁺: [Ar] 4s⁰3d⁹

another example: Ni²⁺

[Ar] 3d⁸

valence electrons of transition metals

if d is full, it doesnt count and look at the other subshells, but if the d isnt full, then it counts.

paramagnetic

an element can be deflected by a magnetic field

there is an unpaired electron

always paramagnetic if there is an odd number

the more unpaired electrons you have, the more paramagnetic you are

diamagnetic

wont get deflected by a magnetic field

all electrons are paired up

ex:Na+

heisenberg uncertainty principle

its impossible to determine, with perfect accuracy, the momentum and the position of an electron simultatneously, this means

pauly exclusion principle

no two electrons in an atom can have the same four quantum numbers

quantum numbers

an electrons address

an atoms absorption spectrum

each atom has a specific absortion spectrum, measures the amount of energy, in the form of photons of light, and thus a change in wavelength was absorbed by the sample

every atom has its own wavelength at which it will absorb energy due to the unique configuration of the electrons in the outer shell.

endothermic when it absorbs energy and electron goes to a higher orbitial

exothermic when the electron releases energy, or emits a photon

E=hc/λ

h=planks constant, 6.626x10^-34

c=light, 3x10⁸

λ=wavelength

einsteins equation-nuclear energy

E=Δmc²

E=energy; Δm=mass; c=speed of light=3x10⁸

in the nuclear reaction, mass is converted into energy-al nuclear reactions convert mass into energy. little mass turns into ALOT of energy.

in nuclear reactions, products will therefore way less than reactants cuz mass has been converted into energy, and they are therefore exothermic.

strong force

protons hate eachother and dont want to be close, so they repel.

they stay in the nucleus becuase there is an attractive force in nucleus called the strong force which overcomes the electrostatic replsion between protons

strong force comes from the nuclear binding energy

nuclear binding energy

protons and neutrons seperately weigh more than when they are put together in the nucleus--they sacrafice some mass and convert to energy so they can hold protons and neutrons in the nucleus. the mass thats converted into energy is the neclear binding energy.

stable nucleus-hgih nuclear binding energy

unstable/radioactive=lower nuclear binding energy

alpha particle

²₄α-2 protons and mass number of 4-2 neutrons

equivalent of helium nucleus, but not same as helium atom because it doesn't have electrons.

proton

¹₁p -has one proton and mass number of one

nuetron

no charge, but a mass number of 1, less than a proton

¹₀n

beta partice

an electron, has -1 charge, and mass number is 0, but it really does have a tiny mass its just rounded

⁰_-1β

positron

positively charged electron and can be emitted out of a nucleus.

⁰₊₁β

gamma

its a photon of light, and it actually does have a 0 mass.

⁰₀ϒ

penetrating power

as mass decreases, penetrating power increases--gamma is most penetrating and will do the most harm, alpha will do the least harm

stable nucleus

1. even number of protons and or neutrons-if odd number of protons and nuetrons, you are probably radioactive-better if neutrons and protons are paired up.nitrogen-14 is exception

2. n/z ratio-want it as close to 1 for lighter elements, after you pass 20, want more neutrons, so higher than 1.-want atom to lie close to belt of stability

n-neutrons; z=protons

3. magic numbers-2, 10, 18 electrons-noble gases with filled shells

nuclear reaction

can invert one element into another element

parent nucleus=reactant

daughter nucleus-product

alpha decay

⁴₂ α as product-put on right hand side of equation

whenever you emit something its a product of that reaction

reduces mass number

every element greater than 83, palonium and higher are radioactive. z>83

β-decay

⁰_-1β

always talking about electron emission, shows up on product side

proton+electron=neutral, mass number=1

when you combine proton and electron, you get a neutron

turns a neutron into a proton by taking out an electron

if you are above belt of stability, n/z ratio is high so you want more protons, so you go thorugh beta decay

electron capture

when inner core electron is sucked into the nucleus

electron is on reactant side of arrow ⁰_-1e

turns a proton into a neutron

have proton in nucleus and sucks in a electron, it makes a neutron by capturing the electron-capture negative electron

if below belt, n/z is too low so there are too many proton and not enough neutrons, so want to turn protons into neutrons by electron capture

positron emission

0+1β

turns proton into a nuetron

gives off a positive electron to make a neutron.

if below belt, n/z is too low so there are too many proton and not enough neutrons, so want to turn protons into neutrons by positron emission

gamma emission

usually accompanies another nuclear process

have nuclear reaction and product nucleus isnt that stable yet so you it emits some high energy light and it gets more stable.

same parents and daughter

About this deck

By: Gerri Blick
Created: 2011-05-21
Size: 42 flashcards
Views: 27

About StudyBlue

“I have used this website for three exams, and I see a huge difference in my test results.”
Naj