Lesson 17

In this lesson, we discovered that some atoms, when set aflame, burn bright colors. Certain properties within the elements cause this spectral sight, and it can be used in experiments to determine if a metal is present in a compound. Strontium compounds will burn a vibrant red, while sodium produces a yellow-orange hue. Copper takes blue-green, while potassium burns either lilac or a light pink. Colors appear only if a metal is present; nonmetals don't give us much to look at.

Problems:
What flame colors would be produced by these compounds? Explain.
a.) Na2CO3 - Yellow-orange, because sodium is present.
b.) Ba(OH)2 - Blue-green...? Barium is present, and that's what color of flame it produces.
c.) KOH -  Pink-lilac! This is one of the substances we tested; potassium gives it its color.
d.) K2CO3 - Pink-lilac again, because of the potassium.
e.) BaO - Blue-green because of the barium in the compound.

Imagine you were in charge of creating a red and purple fireworks display. Name two combinations of compounds you could use.

Strontium, as stated above, produces a vibrant firetruck red color, so you'd probably want some strontium compounds in your firework mix. Lithium would also do, so you could use lithium sulfate. As for the purple fireworks, you could use potassium compounds, since potassium gives off a lilac-y color when burned.