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Nikolay [14]
2 years ago
7

What is a flame test?

Chemistry
2 answers:
Greeley [361]2 years ago
8 0

A flame test is a method of obtaining an emission spectrum from a sample

(4.2.2 Spectra)

Svetlanka [38]2 years ago
5 0

Answer:

B. A method of obtaining an emission spectrum from a sample

Explanation:

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Which of the following equations are correctly balanced
IRINA_888 [86]
Ion know yo but good luck
7 0
3 years ago
In an chemicalbreaction involving Fe and S, it was found that 45.2 g of Fes was produced. If the percent yield of the reaction i
saw5 [17]

Answer:

47.8 g

Explanation:

Remember the equation for percent yield:

% yield = actual / theoretical

We're given two of the values in the question, so plug n' play:

0.945 = 45.2 / theoretical

theoretical = 47.8 g

Keep in mind you can use mass here without converting to moles because we're working with products only. If you were given a mass of reactants, you would need to convert to moles and using a balanced chemical equation find the corresponding moles of product produced.

7 0
3 years ago
What type of circuit is shown in the diagram below?
Rzqust [24]

Answer:

Its a simple SERIES circuit

Explanation:

3 0
3 years ago
Which of the following halogens has the largest atomic radius?
pickupchik [31]

Answer:

\boxed {\boxed {\sf B. \ Iodine }}

Explanation:

Atomic radius is the measurement from the nucleus to the outer edge of the electron cloud.

As you go down a group (vertically) the atomic radius increases because more electron shells are added. As you go across a period horizontally, the atomic radius decreases.  

If we look at the halogens group (17), we see they follow this order from top to bottom:

F - Fluorine

Cl - Chlorine

Br - Bromine

I - Iodine

Since it increases down the group, iodine  must have the largest atomic radius.

4 0
3 years ago
Rank the following five elements by ionization energy Rank from highest to lowest ionization energy. To rank items as equivalent
yan [13]

Answer:

Cl

Si

Mg

Na

Explanation:

Ionization energy is the energy required to remove an electron from the valence shell of an atom to form an ion. Since metal are natural givers, they help people. Non metals are receivers hence it would be very hard for them to release their electrons.

For our arrangement, the key is that the ionization energy is expected to increase across the period to a maximum that terminates at the halogens. This is the more reason why halogens have the highest ionization energy and the alkali metals have the lowest.

Hence, from the options in the question, we can see that chlorine would have the highest because it is an halogen in group 17. Also expected is the fact that the ionization energy of that Mg is greater than that if Na. This is because Mg comes after Na in the same period and is thus expected to have higher ionization energy than Na

7 0
3 years ago
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