Topic
Q:
Draw a Lewis structure for \( \mathrm{SO}_{2} \) in which all atoms obey the octet rule. Show formal charges. Do not consider
ringed structures.
Select Draw
Q:
b. A sample of 50 g of ethanol, increases in temperature from \( 0^{\circ} \mathrm{C} \) to \( 25^{\circ} \mathrm{C} \). What is
the amount of energy absorbed? Specific heat of ethanol is \( 2.42^{\circ / g^{\circ} \mathrm{C}} \)
\[ q=(25)(50)(2.42)=3,025 \mathrm{~J}-0^{\circ}-\mathrm{C}=25^{\circ} \]
Q:
produces \( \mathrm{OH}^{-} \)in water
\( \begin{array}{l}\text { acid } \\ \text { base } \\ \text { both }\end{array} \)
Q:
\( \operatorname{MgBr}_{2} \)
\( \begin{array}{l}\text { acid } \\ \bigcirc \text { base } \\ \text { salt }\end{array} \)
Q:
Which best describes activation energy?A. the maximum amount of energy required to end a chemical reactionB. the amount of energy absorbed in an endothermic reactionC. the minimum amount of energy required to start a chemical reactionD. the amount of energy released in an exothermic reaction
Q:
When I drop blue dye into a beaker full of water the blue dye drop is extremely intense in
color at first, but the water eventually becomes a uniform lighter blue. How does this
scenario relate to diffusion?
Q:
Draw the Lewis structure of carbon monoxide \( (\mathrm{CO}) \) and then determine if the
molecule is polar or nonpolar. Please place the elements in the order that they are
written.
Q:
Draw the Lewis structure of \( \mathrm{CBr}_{4} \) and then determine its electron domain and
molecular geometries.
Q:
35 Metal \( X \) does not react with cold water but does react very slowly with steam
What is the position of \( X \) in the reactivity series?
A sodium \( \rightarrow X \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow \) copper
B sodium \( \rightarrow \) calcium \( \rightarrow X \rightarrow \) magnesium \( \rightarrow \) copper
C sodium \( \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow X \rightarrow \) copper
D sodium \( \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow \) copper \( \rightarrow X \)
Q:
Lattice enthalpy for NaCl is \( +788 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and
\( \Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1} \). Enthalpy of solution of \( \mathrm{NaCl}^{\circ} \) is
\( \begin{array}{ll}\text { (a) }+572 \mathrm{~kJ} \mathrm{~mol}^{-1} & \text { (b) }+4 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \text { (c) }-572 \mathrm{~kJ} \mathrm{~mol}^{-1} & \text { (d) }-4 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array} \)
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