Chem Quiz, lewis dot structure, energetics, naming covalent compds

sublimation

(s) → (g)

Energy required to cause a change of phase from solid to gas: ∆H_sub

endothermic

Ionization energy

Na(g) →Na⁺(g) + e^-

Energy required to remove an electron from a neutral atom or an ion: IE

endothermic

Bond Dissociation Energy

½Cl²(g) → Cl(g)

Energy required to break a chemical bond in a compound: BDE

endothermic

electron affinity

Cl(g) + e^- →Cl^-(g)

Energy released when an electron is added to a neutral atom or an ion.: AE

exothermic

Lattice energy

Ca⁺(g) + 2 Br^-(g) → CaBr₂ (g)

Energy change associated with forming one mole of a solid ionic compound from its gaseous ions: LE

Exothermic

Enthalpy of Formation

(net reaction)

Net change in energy when forming a compound from its elements: ∆H_f

Exothermic

Ionic vs covalent: melting point

Ionic: high

Covalent: low

Ionic vs covalent: element type

Ionic: metal to nonmetal

Covalent: nonmetal to nonmetal

Ionic vs covalent: nature of bond

Ionic: complete transfer of electrons

Covalent: shared electrons

Ionic vs covalent: solubility

Ionic: most are soluble

Covalent: some soluble

Ionic vs covalent: conductivity solution

Ionic: electrolyte

Covalent: non electrolyte

Ionic vs covalent: conductivity of liquid

Ionic: yes when molten

Covalent: no when molten

Exothermic

releases energy

(forms interactions/bonds)

△E = -

endothermic

requires energy

(breaks interactions/bonds)

△E = +

NH₃

ammonia

Covalent naming: 1

mono

Covalent naming: 2

di

Covalent naming: 3

tri

Covalent naming: 4

tetra

Covalent naming: 5

penta

Covalent naming: 6

hexa

Covalent naming: 7

Hepta

Covalent naming: 8

Octa

Covalent naming: 9

nona

Covalent naming: 10

deca