⭐️Periodic Table Flashcards by Tiffany Rhodes

Mendelev

Correctly predicted the properties and masses of unknown elements–element properties were periodic functions of it MASS (wrong bc isotopes)

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Mosely

Properties of element are a periodic function of it ATOMIC NUMBER (right)

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Horizontal on periodic table

Periods/rows

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Vertical on periodic table

Groups/columns/families

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Families in a periodic table

More similar chemical properties than periods, same # of valance electrons

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Higher atomic radius effects

More QUANTUM LEVELS, weaker nuclear pull, down a group, shielding effect, IE decreases, ionization decreases, affinity decreases

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Covalent atomic radius

1/2 inter-nuclear distance between 2 adjacent atoms in a SOLID phase, in Angstroms

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How many angstroms are in a meter

10^-10

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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)

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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)

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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)

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Ionic radii, bigger in nonmetals or metals?

Size of an ion’s radius, bigger in nonmetals (gain)

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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)

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Within a period, as atomic number increases, density…

Increases, then decreases

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Period

Same quantum/energy level, decreasing radius, increasing nuclear pull/ionization/affinity

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Within a family, going down, density…

Generally increases

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Within a family, what happens to melting point?

Increases, then decreases in groups 1 and 2

Increases for other groups

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Ionization energy (IE)

Amount of ENERGY needed to REMOVE the most loosely bound electron, forming a cation

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Within a group, going down, what happens to IE/Affinity?

Decreases (less energy needed to lose furthest electron) MORE SHIELDING EFFECT, LOWER NUCLEAR PULL

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Within a period, going across, what happens to IE/Affinity?

Increases (greater energy needed to remove furthest electron) MORE VALANCE ELECTRONS, STRONGER NUCLEAR PULL

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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)

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Electron affinity

Attraction an atom has for electrons (when non-bonded) [thats also why nonmetals gain, more nuclear pull, easier to gain than lose]

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As radius decreases what happens to ionization/affinity

Inverse, increases

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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

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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)

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

⭐️Periodic Table Flashcards

(69 cards)