Draw the Lewis structure for hydrogen sulfide, $\mathrm{H}_2 \mathrm{~S}$.

What type of bonding would be expected between the following atoms? a. Li and F, b. Cu and S, c. I and Br

How did Max Weber define power?

How to draw a Lewis structure of NO${_3^-}$ ion?

How to draw a Lewis structure for H$_3$O$^+$ ion?

Draw the Lewis structure for chloroform, $CHCl _9$. What are its electron-pair and molecular geometries? What orbitals on $C, H$, and $Cl$ overlap to form bonds involving these elements?

Draw the Lewis structures for the following molecules: a. IBr, b.

$$\mathrm { CH } _ { 3 } \mathrm { Br }$$

, c.

$$\mathrm { C } _ { 2 } \mathrm { HCl }$$

, d.

$$\mathrm { siCl } _ { 4 }$$

, e.

$$\mathrm { OF } _ { 2 }$$

Name the compound HBr and classify it as either ionic or molecular. Is it a strong acid, a weak acid, a strong base, or a weak base?

How many digits after the decimal point should be reported when the calculation $(10.434-9.3344)$ is performed?

If $\ce{[H3O+]} = \pu{7.5E-9 M}$ for a particular solution, what is the pH?

Which of the following are Arrhenius bases?

• a) LiOH
• b) Ba(OH)$_2$
• c) Al(OH)$_3$
• d) All of these are Arrhenius bases.

Why is the Arrhenius acid-base definition too limited? Give an example for which the Arrhenius definition does not apply.

Draw the Lewis structure of phosphorus trifluoride, $\mathrm{PF}_3$. One molecule has $\square$ P atom(s) and $\square \mathrm{F}$ atom(s).

Each $P$ atom has $\square$ valence electrons.

Each $\mathrm{F}$ atom has $\square$ valence electrons.

There are $\square$ valence electrons available for bonding.

Use the space at the right to arrange the $P$ and $F$ atoms, using dots to represent electron pairs and lone pairs. Make sure the final result contains the same number of dots as there are valence electrons available for bonding.

Draw a Lewis structure for silane $\left(\mathrm{SiH}_4\right)$, and predict its molecular geometry.