U2 Exam

P. Trends

100

Which element is larger in radius: Mg or N

Mg

200

Which element is more electronegative: O or P

O

300

Rank the following elements from big to small: 

N, Mg, S, Ge

Ge, Mg, S, N

400

Explain the trend for radius across the period (L to R).

more protons=strong magnet=Shrink

500

Explain the trend for electronegativity across the period (L to R)

Increases. more val e on outer shell = affinity for electrons is stronger

Types of Solids

100

Which type of solid contains IMFs (intermolecular forces)?

molecular covalent

200

Why do molecular covalents have a lower melting point than ionic solids?

IMF's (forces) holding molecule together, therefore not as much energy needed to pull apart

300

List 3 properties of ionic solids  

dissolve

conductive when dissolved

brittle

crystalline

400

Explain why H₂ is nonpolar covalent?

equal sharing of electrons

500

Give an example of a polar molecule. 

Answers may vary

Naming

100

Name the following ionic compound: NaCl

Sodium Chloride

200

Name the following covalent compound: N₂O₃

dinitrogen trioxide

300

Name the following ionic compound: Fe₂O₃

Iron (III) oxide

400

Write the formula for the following acid: sulfurous acid

H₂(SO₃)

500

Write the formula for the following: chromium (III) carbonate

Cr₂(CO₃)₃

Ionic Lewis Structures

100

List two elements that have 6 valence electrons.

Elements from group 16

200

List two elements that make a 3- ion.

Elements from group 15

300

Draw the ionic lewis structure for MgF₂

answers vary

400

What is the chemical formula for magnesium bonded with nitrogen? 

Mg₃N₂

500

What is the chemical formula for sodium bonded with hydroxide?

Na(OH)

Covalent Lewis Structures

100

Draw the lewis structure for water.

See student picture

200

Draw the lewis structure for N₂

see student picture

300

What is the angle between electron groups in a tetrahedral?

109.5^o

400

What is the molecular geometry H₂S

bent

500

what is the molecular geometry of PH₃

trigonal pyramidal