Unit 2 Quiz IMFs and Properties Quiz

Metallic Solids are made up of

atoms just from metals

Molecular solids are made up of

nonmetals and are relatively small

Covalent Network Solid is made up of

a large structure of covalently bonded atoms, nonmetals

ionic solids are made up of

a combination of metal and nonmetal atoms

Properties of ionic Solids

• High melting point

• Low vapor pressure(due to high IMFs)

• Brittle

• Poor conductors(rigid structure, not fluid)

• Can be conductors when liquid

• Can be broken down in solutions using water

Metallic Solids Properties

• Many free moving electrons

• Shiny

• good conductors(due to many free electrons)

• Ductile(Atoms are able to move and stretch out)

• Malleable(protons have the ability to move)

• Can form alloys

  • interstitial and substitutional

Alloys

melting different metals to derive different characteristics in order to create a metal with new characteristics

Interstitial alloys

• Alloying smaller atoms to fill in the holes between larger atoms

• Ex: steel

• this increases density, making it a better metal

Substitutional Alloys

• replacing atoms with another atom that is around the same size

• Ex: Brass

• keeps around the same density/mass

Covalent network solids properties

• made up of either one non-metal or 2 non-metals

• generally made from the carbon group due to the 4 valence electrons that allow it to make a vast # of bonds

• either 2D or 3D structure

• high melting point due to high amount of bonds

• Held together by LDFs(weak so layers are able to slide past one another)

Molecular Solids Properties

• include:

  • Nonmetals(sulfur)

  • diatomic elements(HCL)

  • compounds(salt, sugar)

• good insulators(highly structured, meaning less free electrons to conduct electricity)

• Weak IMFs

• Low melting point

intramolecular

Forces within the molecules themselves

Intermolecular

Forces between molecules

London dispersion Forces(LDFs)

attractive forces between molecules(IMFs) that are created by uneven electron distributions that create dipoles/temporary dipoles

increase in contact area between molecules =

increase in LDFs(more es close to eachother)

increase polarizability =

increase in LDFs and molecular size

increase in pi bonding will also

incrs. LDFs

polarizability

“squishiness” of an atom; an atoms ability to distort its electron cloud when subjected to external electric field

Dipole-dipole force definition

interaction between 2 dipoles

3 forms of a hydrogen bond:

H-F; H-N; H-O

Induced Dipole

something that is not polar but can be for a second(polarizable)

Dipole-ion interaction example

using water to break down salt(using dipoles to break down solutions)

Greater IMFs(in liquids/solids) causes(list properties it affects)

• HIGHER melting/boiling point

• GREATER surface tension

• GREATER adhesion(attraction to surrounding container)

• LOWER vapor pressure

Viscosity =

how easily a liquid is able to flow

Describe the key features of a heat curve

flat line = transition phase (combination of the 2 phases it is between)

increasing slope = the current phase the substance is at

light noble gases will have ______ speed compared to ______ gases

higher speed; heavier gases

Pressure vs. Volume

increase pressure = decrease volume

Volume vs. Temperature

increase temperature = increase volume

Volume vs. moles

increase moles = increase volume

n = PV/RT always equals ____

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