Day 2: Periodic Trends and Bonding

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

Metals _____ electrons

Back (Answer)

lose

Front (Question)

Non-Metals_____ electron

Back (Answer)

gain

Front (Question)

Z-S =Zeff

Back (Answer)

Greater Zeff = smaller the atomic radius. Electrons are held closer to nucleus

Front (Question)

Ionic radius increases

Back (Answer)

Down and to the left France has wine & cheese = Fr biggest atomic radius

Front (Question)

Isoelectronic series

Back (Answer)

Most (+) smallest radius Most (-) largest radius

Front (Question)

1st Ionization energy

Back (Answer)

Energy needed to remove an electron from the first shell endothermic oxidation **Exceptions - B, O, N)

Front (Question)

Electron affinity

Back (Answer)

energy change associated with gaining an electron Trend: to the right ( more (-)) Ionic bonding Exothermic Reduction

Front (Question)

Electronegativity

Back (Answer)

Increases up and to the right Covalent bonding Exceptions: Be/N

Front (Question)

More polar bond

Back (Answer)

Bigger electronegativity difference

#10

Front (Question)

Covalent network solids

Back (Answer)

Diamond & Quartz non-metal with non-metal Sharing e-

#11

Front (Question)

Ionic (ionic crystals)

Back (Answer)

metal with non-metal crystaline, high melting/boiling point brittle

#12

Front (Question)

Metalic (metalic lattices)

Back (Answer)

metal with metal Valance e- loosely held Electrical/thermally conductive Ductile- draw them into wires easily & malleable luster/shiny high melting/ boiling point

#13

Front (Question)

Molecular

Back (Answer)

lower m.p. & b.p. 2 non-metals

#14

Front (Question)

Lewis dot structures

Back (Answer)

***Exceptions: CH4, CO2, SF4)

#15

Front (Question)

Polar covalent bonds

Back (Answer)

electrons shared by the atoms spend a greater amount of time, on the average, closer to the more electronegative atom, causing a dipole

#16

Front (Question)

Coordinate covalent bonds

Back (Answer)

A covalent bond is formed by two atoms sharing a pair of electrons. The atoms are held together because the electron pair is attracted by both of the nuclei. Lewis base & Lewis Acid NH3 + HCl –> NH4Cl

#17

Front (Question)

Exceptions to the octet rule

Back (Answer)

H -2 Be- 4 B- 6 Al- 6 Can exceed octet- 3rd row or lower odd #

#18

Front (Question)

Atoms on the left of the fisher projection

Back (Answer)

Axial position

#19

Front (Question)

Atoms on the right of the fisher projection

Back (Answer)

Equatorial position Lone pairs are put here due to large repulsion

#20

Front (Question)

Hybirdization

Back (Answer)

Electrons are promoted (sp, sp2, sp3, sp3d, sp3d2)

#21

Front (Question)

Electron domain - 2 non bonding pairs of e- = 0

Back (Answer)

sp 180 degrees Electron Geometry -linear Molecular Geometry- linear

#22

Front (Question)

Electron domain - 3 non bonding pairs of e- = 0

Back (Answer)

sp2 120 degrees EG- Trigonal planar MG- Trigonal planar

#23

Front (Question)

Electron domain - 3 non bonding pairs of e- = 1

Back (Answer)

sp2 120 degrees EG- Trigonal planar MG- Bent

#24

Front (Question)

Electron domain - 4 non bonding pairs of e- = 0

Back (Answer)

sp3 109.5 dgrees EG- Tetrahedral MG-tetrahedral