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PR - Big book > 25.1-25.10 > Flashcards

25.1-25.10 Flashcards

1
Q

alpha decay

A

alpha is the biggest (2 protons 2 neutrons)

alpha particle can be stopped by human skin

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2
Q

beta decay (three types)

A

proton to neutron (vice versa)

Beta-

Beta+

Electron capture

stronger than Alpha particle, but can be stopped by aluminum foil

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3
Q

Beta- decay (Standard BETA decay)

A

unstable nucleus has TOO MANY NEUTRONS

converts neutron to proton and electron

atomic number UP by 1, mass stays the same

Ca -> Sc + 0 -1 beta

what is emitted?

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4
Q

Beta+ decay (positron emission)

A

too few neutrons

proton becomes a neutron and a positron (identical to electron but with a positive charge)

atomic number DOWN by 1, no change in atomic mass

Co -> Fe + 0 +1 beta

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5
Q

electron capture

A

converts a proton into a neutron by capturing an electron

no change in mass number, but atomic number DOWN by 1

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6
Q

gamma decay

A

often accompanies other kinds of decay

stopped by lead or concrete

“gamma lead”

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7
Q

nuclear bind mass

A

LOSES mass when nucleus is formed

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8
Q

kilograms in an amu

A

1.66 ( 10^-27) kg

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9
Q

equation for nuclear binding energy

A

deltaMass (in amu) * 931.5 MeV

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10
Q

equation for energy of photon

A

E = hf

“Photons just wanna Have Fun”

fun is speed of c / wavelength

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11
Q

Planck’s constant

A

6.63 * 10^-34

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12
Q

electron has more energy when farther from nucleus!

A

like potential energy

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13
Q

En = (-2.178 * 10^-18) / n^2

A

Change in energy = E_final (n=1) - E_starting (n=2,3)

negative means energy is RELEASED

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14
Q

Bohr model contains 1 electron

A

1 ELECTRON = BOHRING

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15
Q

the p orbitals are like dumbbells

A

3 x,y,z

d has 5 orbital configurations (p has 3)

f has 7 orbital

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16
Q

diamagnetism/paramagnetism

A

diamagnetism - all electrons are spin paired

REPELLED by externally produced magnetic field

paramagnetism - not all spin paired (“WEIRDLY uneven”)

attracted into externally produced magnetic fields

17
Q

PERIOD and GROUP (and block)

A

PERIOD HORIZONTALLY (periods are like elipses…)

GROUP VERTICALLY (groups are like columns, stacks)

there are 4 blocks (s, p, d, f)

subtract 1 for d from period

subtract 2 for f from period

18
Q

3d

A

subtract down 1

4s2 3d10 …

THE FIRST D ROW IS ACTUALLY 3

19
Q

EXCEPTIONS: Chromium and Copper electron configuration

A

FILL the d orbitals (4->5, 9->10)

20
Q

EXCEPTIONS: Ag and Au

A

9->10
Ag = silver
Au = gold

FILL the d orbitals

21
Q

isoelectronic

A

iso = same electric shape

F- and Neon (same e- configurations)

22
Q

Transition metals lose s electrons before they lose d electrons

A

IMPORTANT - the s is valence electron since n > n-1

Transition metals are elements in the d block

ex. Ti is [Ar] 4s2 3d2

Ti2+ is [Ar] 3d2

23
Q

first two groups

A 
Alkali metals (1 word)
Alkaline earth metals (2 words)
24
Q

halogens are powerful oxidizing agents

A

x

25
Q

Metalloids

A

B Si Ge As Sb Te Po

26
Q

atomic radius DECREASES going left to right (Zeff is higher to the right)

A

also decreases going up

27
Q

X+ < X < X-

A

cations are smaller than anions

28
Q

ionization energy = energy to remove an electron

A

INCREASES going right – valence electrons are more tightly bound

the 2nd ionization energy is always more than the 1st

29
Q

electron affinity

A

halogens are VERY affinitive (energy is released = negative, increased stability)

Very POSITIVE for noble gases and ALKALINE EARTH METALS because they need a new level or sublevel and this destabilizes (“they really don’t want more electrons”)

affinities increase going RIGHT and UP (a general trend, does not include noble gases)

30
Q

electronegativity

A

pulls electrons when forming a covalent bond (unfair sharing)

F > O > N/Cl > Br > I > S > C/H

31
Q

formal charge

A

valence electrons - 1/2 (electrons in bonds) - lone electrons

32
Q

resonance structures

A

nonbonding electrons, double and triple bonds can move around

33
Q

coordinate covalent bond

A

lone pair forms a bond on its own (obtains a formal positive charge) = LEWIS BASE

LEWIS BASE = NUCELOPHILE

LEWIS ACID = ELECTROPHILE = accepts electrons

34
Q

coordinate covalent bond

A

lone pair forms a bond on its own (obtains a formal positive charge) = LEWIS BASE

LEWIS BASE = NUCLEOPHILE

LEWIS ACID = ELECTROPHILE = accepts electrons

35
Q

oxidation states p. 668

A

keep working on it

PR - Big book (29 decks)

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