⭐️Periodic Table Flashcards
Mendelev
Correctly predicted the properties and masses of unknown elements–element properties were periodic functions of it MASS (wrong bc isotopes)
Mosely
Properties of element are a periodic function of it ATOMIC NUMBER (right)
Horizontal on periodic table
Periods/rows
Vertical on periodic table
Groups/columns/families
Families in a periodic table
More similar chemical properties than periods, same # of valance electrons
Higher atomic radius effects
More QUANTUM LEVELS, weaker nuclear pull, down a group, shielding effect, IE decreases, ionization decreases, affinity decreases
Covalent atomic radius
1/2 inter-nuclear distance between 2 adjacent atoms in a SOLID phase, in Angstroms
How many angstroms are in a meter
10^-10
Within a PERIOD, what happens to the size of the radius with increasing atomic number?
Decreases (going across), up atomic number, more protons, more electrons in the same energy level, higher nuclear charge, stronger nuclear pull EXCEPT NOBLE GASES ARE SLIGHTLY LARGER (as compared to elements near it)
Within a FAMILY, what happens to the size of the radius with increasing atomic number?
Increases (going down), each row has increasing energy levels, weaker nuclear pull (shielding effect)
Non-metals gain electrons, (-) ions (anion)
It’s radius will be LARGER, therefore WEAKER nuclear pull (more electrons out there, less pull bc can’t pull so many)
Ionic radii, bigger in nonmetals or metals?
Size of an ion’s radius, bigger in nonmetals (gain)
Metals lose electrons, (+) ions (cation)
It’s radius as an ion will be SMALLER, therefore STRONGER nuclear pull (since there’s less electrons to pull the pull is stronger)
Within a period, as atomic number increases, density…
Increases, then decreases
Period
Same quantum/energy level, decreasing radius, increasing nuclear pull/ionization/affinity
Within a family, going down, density…
Generally increases
Within a family, what happens to melting point?
Increases, then decreases in groups 1 and 2
Increases for other groups
Ionization energy (IE)
Amount of ENERGY needed to REMOVE the most loosely bound electron, forming a cation
Within a group, going down, what happens to IE/Affinity?
Decreases (less energy needed to lose furthest electron) MORE SHIELDING EFFECT, LOWER NUCLEAR PULL
Within a period, going across, what happens to IE/Affinity?
Increases (greater energy needed to remove furthest electron) MORE VALANCE ELECTRONS, STRONGER NUCLEAR PULL
How can u tell if an element has no affinity
If the first ionization energy makes a big jump and the valence is full or sublevel p, d, or f is 1/2 full (s2 p3 p6 d5 d10 f7 f14)
Electron affinity
Attraction an atom has for electrons (when non-bonded) [thats also why nonmetals gain, more nuclear pull, easier to gain than lose]
As radius decreases what happens to ionization/affinity
Inverse, increases
How can u tell which group the element is in based on IE?
Big jump, new quantum level, previous quantum level=valence, valence=group…for example
X+1>X+2=1810 KJ
X+2>X+3=2750 KJ
X+3>X+4=11000 KJ…big jump, 3 valence, group 13
Metals (where on p table, properties, lose or gain electrons/where, how many valence)
2/3 of periodic table, left of red line (not H), luster malleability high melting point good conductors low IE, low affinity, lose electons (easily loses down bc shielding and left bc weaker nuclear pull) 1 2 3 valence
What is the most active metal/most metallic
Francium, 1 valance in 7th level (only needs to lose 1)
Within a period, metallic properties…
Decreases (higher nuclear charge)
Within a family, metallic properties…
Increase (higher shielding)
Non-metals (where on p table, properties, lose or gain electrons/where, how many valence)
1/3 of periodic table, dull low mp high IE, gain electrons (easier gains bc less shielding and stronger nuclear pull), 5 6 7 valence
What is the most active non-metal
Flourine (has 7 valence needs 1 more)
Metalloids (what and where?)
Generally touching red line (NOT Al, Po, or At) includes B Si Ge As Sb Te
Group 1
Alkali metals, 1 v, +1 (needs to lose 1 valence to become a noble gas i.e. Rb+1=Kr) MOST ACTIVE
•not found in nature found as compounds (ionic) i.e. Na+1 Cl-1 > NaCl
•For electrolytes (electrochemical signals) for body
Group 2
Alkaline Earth Metals, 2 v, +2 (loses max of 2e, +2), active but not as active as alkali, found as compounds i.e. Mg+2 Cl2-1 > MgCl2
Groups 3->12
Transition metals, filling in d sublevel (d block, meaning the highest energy sublevel is d), multiple oxidation states, form colors in solution (no color in Zn bc 3d10 is full)
How many electrons are in the sublevels before the first d (3d)
20
Group 13
3 v, +3
Group 14
4 v, (don’t have to know oxidation), C is an allotrope
Group 15
5 v, -3, N is an allotrope
Group 16
Chalcogens, 6v, -2
Group 17
Halogen (contains elements w all 3 phases @ room temp), 7 v, -1
Group 18
Noble/intert/monatomic gas, full v (octate 8 v besides He), no affinity
When ur in the bottom left corner ur gonna…
Lose a little metallically and be quite dense generally, you’ll be quite big but pretty weak, your shielding effect is pretty neat, so you won’t need much ionization energy or have a lotta affinity!
When ur in the top right corner of the periodic table…
You’re a nonmetal so you’ll gain a lot, ur not quite dense ur such a thot, ur pretty small but pretty spicy, strong, and hot, barely any levels.. bitch that’s what u got, you need a lotta ionization energy to lose yo dots!
Allotropes
Different forms for an element in the same phase, C N P O
Lanthanides/actinides
F-block, more similar next to eachother
When u got a diagram and are in doubt…
Figure out wt element it is (count electrons) and go to periodic table
The size of an element is determined by…
X-Ray refraction of a crystal of the element
A low ionization is characteristic of a…
Metal
Ionization energy increases as u…
Go up and right
Size of radius increases as u…
Go down and left
When metallic atoms lose electrons, do they form smaller or larger ions than the original atom?
SMALLER because STRONGER nuclear pull (since there are less electrons to pull)
When nonmetallic atoms gain electrons, do they form smaller or larger ions than the original atom?
LARGER because WEAKER nuclear pull (since there are more electrons to pull)
When forming compounds, the combined elements must have…
A noble gas configuration (ions cancel out…ex 1- and 1+)
If there are 1 2 or 3 total valence electrons, does the atom lose (+) or gain (-) electrons?
LOSES (+) the amount that it needs to get to the previous sublevel
If there are 5 6 or 7 total valence electrons, does the atom lose (+) or gain (-) electrons?
GAINS (-) the amount it needs to get to the next sublevel
Which elements are liquid at STP?
Bromine and Mercury
Carbon allotropes
SOLID coal, graphite, diamond, graphene, carbon nanotubes
Nitrogen allotrope
GAS
N2=atmosphere
N3=Azide
Phosphorus allotrope
SOLID
White=explodes in air
Red=matches, stable until friction
Black=in computers, semiconductors, stable
Oxygen allotropes
O2=air
O3=ozone
Lanthanides and Actinides
Within rows 6 and 7, filling in F sublevel (f block)
Within a PERIOD, why does affinity increase?
Smaller radius, greater nuclear PULL…not smooth, some have full/half full valence
Within a FAMILY, why does affinity decrease?
Increased shielding, less nuclear PULL/attraction for electrons, larger RADIUS
Across a row, the radius of ions…
Decrease (lose 1-3v) than increase (gain 5-7v)
As you move across transition metals in the 5th row, what energy level are additional atoms placed in?
4th (use diagonal rule shortcut) Row 5= 5s1, 5s2, transition starts at 4d1
Chalcogens
Group 16
Going down a group, radius is affected by…
OF QUANTUM LEVELS
Going down a group, IE/Affinity is affected by…
SHIELDING AFFECT
(Write out this problem to answer) For an atom in 3rd period
A) p orbital can be partially full
B) 2nd principle energy level is not full
C) more than 6 complete orbitals
A, draw out Na (the minimum configuration for row 3) only has 3 complete orbitals, 2nd principle energy level (2s and 2p) is full, but the p level CAN be partially full if we keep going
