A radioactive tracer, I believe. Someone check that lol.
Answer:
Types of atomic orbitals present in the third principal energy are <u>s, p and d only .</u>
Explanation:
- <u>OPTION A-: s and p atomic orbitals -</u> these two orbitals are present in second principal energy level. Therefore , the option is incorrect.
- <u> OPTION B-: p and d only -</u> This option is wrong as there is no such principal level energy where , s atomic orbital is absent .
- <u>OPTION C-: s , p and d only -</u>these orbitals are present in<u> third principal energy level</u>. The third major level of energy has one orbital, three orbitals of p, and five orbitals of d, each of which can contain up to 10 electrons. The third stage thus holds a maximum of 18 electrons. This option is correct .
- <u>OPTION D-: s , p, d and f only -</u>There is also a f sublevel at the <u>fourth and higher stages,</u> containing seven f orbitals, which can accommodate up to 14 electrons at most. Therefore, up to 32 electrons will hold the fourth level: 2 in the s orbital, 6 in the three p orbitals, 10 in the five d orbitals, and 14 in the seven f orbitals. This option is incorrect .
<u>Thus , the correct option is C (s , p and d only .)</u>
Answer:
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Explanation:
Answer:
Explanation:
The<em> heat</em> to <em>vaporize</em> a l<em>iquid</em> is equal to the amount of liquid in moles multiplied by the specific <em>heat of vaporiztion</em> per mole.
First, calculate the number of moles in 35.5g of <em>butane</em>.
- Molar mass of butane: 58.124 g/mol
- Number of moles = mass in grams/molar mass
- Number of moles = 35.5g / 58.124g/mol = 0.6107632mol
Now, calculate the heat to vaporize that amount of <em>liquid butane</em>:
- Heat = number of moles × specific heat of vaporization
- Heat = 0.6107632mol × 21.3kJ/mol = 13.0 kJ
The answer must be reported with 3 significant figures.
The empirical formula of the compound is SiCl₄.
<h3>Empirical formula of the compound</h3>
mass of silicon = 28 g/mol
mass of chlorine = 35.5 g/mol
<h3>molar ration: </h3>
Si = 8.56/28 = 0.306
Cl = 43.2/35.5 = 1.216
<h3>Combining ratio</h3>
Si = 0.306/0.306 = 1
Cl = 1.216/0.306 = 4
empirical formula = SiCl₄
Thus, the empirical formula of the compound is SiCl₄.
Learn more about empirical formula here: brainly.com/question/1603500
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