Unit 2

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

Card preview (24)

Front (Question)

Bonds

Back (Answer)

Atoms bond in order to reach a stable 8 valence state

Front (Question)

Ionic Bond

Back (Answer)

Electrostatic forces held together ions. Generally between metals and nonmetals

Front (Question)

Metallic Bond

Back (Answer)

Bons between metals that are neither covalent or ionic: the e- is delocalized so they are free to roam - like a soup

Front (Question)

Covalent Bond

Back (Answer)

Sharing electrons and forming a molecule generally non-metal and non-metal

Front (Question)

Lattice

Back (Answer)

structure of a molecule

Front (Question)

Network covalent bonds

Back (Answer)

Lattice of covalent bonds making a 3D structure

Front (Question)

What are some characteristics of Ionic Bonds (3)

Back (Answer)

• Strong lattice structure • Solid at room temp • High melting and boiling points

Front (Question)

What are some factors for melting points? (2)

Back (Answer)

• Greater charge = greater melting point • Smaller size = greater melting point

Front (Question)

What are some factors for bond energies? (3)

Back (Answer)

• Greater charge = greater bond energy • Smaller size = greater bond energy • More bonds = higher energy (Greater bond order)

#10

Front (Question)

What are some characteristics of metallic bonds? (2)

Back (Answer)

• malleable and ductile • they can form alloys

#11

Front (Question)

Alloy

Back (Answer)

combination of elements where at least one is a metal

#12

Front (Question)

What are the two types of Alloys and explain

Back (Answer)

• Interstitial alloy - different radii sizes • subsitual alloy - similar radii sizes

#13

Front (Question)

What are some characteristics of Network Covalent structures? (2)

Back (Answer)

• Hard • High melting and boiling points

#14

Front (Question)

Aqueous

Back (Answer)

a substance put in H2O

#15

Front (Question)

Bond Order:

Back (Answer)

(total # of bonds)/(# of atoms)

#16

Front (Question)

What are the three rules to keep in mind when you draw Lewis Dot Structures?

Back (Answer)

• Least Electronegative = central atom • Add extra e- till valence shells are finished • Add extra e- to central atom

#17

Front (Question)

What is the maximum amount of e- the central atom can have?

Back (Answer)

No more than 12 They can take up to 12 due to the d-block

#18

Front (Question)

Resonance Forms

Back (Answer)

A bond can go anywhere - in reality, the e- is at all of those locations the equal amount of time

#19

Front (Question)

Incomplete Octets (2)

Back (Answer)

• B and Al - stable with 6 e- • H - stable with 2 e-

#20

Front (Question)

Expanded octets

Back (Answer)

there can be up to 12 e- ONLY AND ONLY IF n = 3 NEVER n = 2 n = 1

#21

Front (Question)

Formal Charge

Back (Answer)

(# of valence e-) - (# of valence e- assigned) PER ATOM

#22

Front (Question)

How do I know if an atom is stable?

Back (Answer)

If the formal charge per atom is 0 or close to 0

#23

Front (Question)

VSEPR

Back (Answer)

Valence electron model that predicts the three dimensional geometry of the molecule

#24

Front (Question)

For formal charge, a lone pair stands for

Back (Answer)

2 e-