4.1 Section Assessment
Q1. Atoms were indivisible and indestructible.
Q2. Using experimental methods, Dalton transformed Democrituss ideas on
atoms into a scientific theory.
Q3. They are observable under scanning tunneling microscopes.
Q4. Atoms are the s
7.3 Section Assessment
Q23. A sea of electrons.
Q24. They are arranged in very compact and orderly patterns.
Q25. Their properties are often superior to that of their component elements.
Q26. Ductility is that metals can be drawn into wires, or changed in
8.1 Section Assessment
Q1. Molecular compounds tend to have relatively lower melting and boiling
points than ionic compounds.
Q2. It shows how many atoms of each element a molecule contains.
Q3. Helium, neon, argon, krypton, xenon, and radon. These are mo
Q1a. sulfide ion, S2b. aluminium ion, Al3+
Q2a. lost 2
b. gained 3
c. lost 2
7.1 Section Assessment
Q3. By looking at its group number
Q4. Atoms of metal tend to lose electrons, while atoms of non-metals tend to gain
or share electrons.
8.3 Section Assessment
Q23. Just as an atomic orbital belongs to a particular atom, a molecular orbital
belongs to a molecule as a whole.
Q24. The repulsion between electron pairs causes molecular shapes to adjust so
that the valence-electron pairs stay a
Week 12 Chemistry
Q1a. Anion, selenide ion
b. Cation, barium ion
c. Anion, phosphide ion
Q2a. Lost 3
b. Gained 2
c. lost 1
9.1 Section Assessment
Q3. When the metals in groups 1A, 2A, and 3A lose electrons, they form cations
Week 16 Chemistry
Q1. Sodium reacts with water to produce aqueous sodium hydroxide and
Week 13 Chemistry
9.3 section Assessment
Q20. A prefix in the name of a binary molecular compound tells us how many
atoms of an element are present in each molecule of a compound.
Q21. Use the prefixes in the name to tell you the subscript of each element
Week 14 Chemistry
Q34. Compound A 2.98gL/0.461gO=6.464gL/1.00gO
Compound B 9.89gL/0.763gO=12.962gL/1.00gO
9.5 Section Assessment
Q35. The law of definite proportions and the law of multiple proportions.