Answer: It is more difficult to remove a valence electron from a Chlorine (Cl) atom
Explanation:
Ionization energy is the energy required to remove the valence electron from an isolated gaseous atom.
Magnesium (Mg) is the 12th element of periodic table and has an atomic number of 12. The electronic configuration is 2, 8, 2. It can easily lose its valence 2 electrons to attain stable configuration.
Chlorine (Cl) is the 17th element of periodic table and has an atomic number of 17. The electronic configuration is 2, 8, 7. It has a tendency to gain electron to attain stable configuration. It cannot lose its valence electron easily as the valence electrons experience more nuclear charge.
Thus it is more difficult to remove a valence electron from a Chlorine (Cl) atom
Chlorine(Cl) is the more difficult to remove a valence electron from which is
because it needs one electron to achieve a stable octet configuration.
Magnesium (Mg) is an element which has an atomic number of 12. The
electronic configuration is 2, 8, 2. This means it has to lose its 2 valence
electrons needed to attain a stable octet configuration.
Chlorine (Cl) is an element which has an atomic number of 17. The electronic
configuration is 2, 8, 7. This means it has to gain one valence electrons
needed to attain a stable octet configuration.
Thus it is more difficult to remove a valence electron from a Chlorine (Cl)
atom than Magnesium atom.
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The density of gold is 19.3 g/cm³. Which of the following shows the mass of a gold bar that is 4.50 cm × 8.00 cm × 20.00 cm?
Answer:
13896g
Explanation:
volume = 4.50×8.00×20.00 = 720 cm³
mass = density × volume
mass= 19.3 × 720 = 13896g
2055 Q. No. 10^-2
mole of KOH is dissolved in 10 litres of
water. What will be the pH of the solution?
12
Ans: pH = 11
Answer:
11
Explanation:
Moles of KOH = [tex]10^{-2}[/tex]
Volume of water = 10 liters
Concentration of KOH is given by
[tex][KOH]=\dfrac{10^{-2}}{10}\\\Rightarrow [KOH]=10^{-3}\ \text{M}[/tex]
[tex][KOH][/tex] is strong base so we have the following relation
[tex][KOH]=[OH^{-}]=10^{-3}\ \text{M}[/tex]
[tex]pOH=-\log [OH^{-}]=-\log10^{-3}[/tex]
[tex]\Rightarrow pH=14-3=11[/tex]
So, pH of the solution is 11
In a lab, you produce a quantity of the radioactive isotope thorium-234. Over the course of several weeks, the unstable isotope decays, and you measure the amount of thorium-234 remaining in the sample. You obtain the following data. What is the half life of Thorium-234? How much Thorium 234 will there be after two half lives?
Days Elapsed Grams of Thorium 234 Remaining
0 16
12 11
24 8
36 6
a. 36 days
b. 12 days
c. 24 days / 4 grams
Answer:
Option C. 24 days / 4 grams
Explanation:
From the question given above, the following data were obtained:
Days Elapsed >>>> Mass Remaining
0 >>>>>>>>>>>>>>> 16
12 >>>>>>>>>>>>>>> 11
24 >>>>>>>>>>>>>>> 8
36 >>>>>>>>>>>>>>> 6
A. Determination of the half-life of Thorium-234.
To determine the half-life, it is important to know the definition of half life.
Half-life is defined as the time taken for a substance to reduce to half its original mass.
From the table given above, we can see that the original mass of the isotope is 16 g (i.e at 0 day). By day 24, the mass of the isotope is 8 g (i.e half the original mass). Thus, the half-life of the isotope is 24 days.
B. Determination of the mass of the isotope remaining after 2 half lives.
Original amount (N₀) = 16 g
Number of half-lives (n) = 2
Amount remaining (N) =?
N = 1/2ⁿ × N₀
N = 1/2² × 16
N = 1/4 × 16
N = 4 g
Thus, 4 g of the isotope is remaining after 2 half lives.
Summay:
Half-life = 24 days
Amount remaining after 2 half-lives = 4 g
Option C gives the correct answer to the question.
Element X has two naturally occurring isotopes, 65X (isotopic mass 65.0457 amu, abundance 20.53%) and 67X (isotopic mass 66.9704 amu, abundance 79.47%). Calculate the atomic mass of element X.
Answer:
66.5753 amu
Explanation:
From the question given above, the following data were obtained:
Isotope A (⁶⁵X):
Mass of A = 65.0457 amu
Abundance of A = 20.53%
Isotope B (⁶⁷X):
Mass of B = 66.9704 amu
Abundance of B = 79.47%
Atomic mass of X =?
The atomic mass of X can be obtained as follow:
Atomic mass = [(mass of A × A%)/100] + [(mass of B × B%)/100]
= [(65.0457 × 20.53)/100] + [(66.9704 × 79.47)/100]
= 13.3539 + 53.2214
= 66.5753 amu
Therefore, the atomic mass of X is 66.5753 amu.
Element X, with an atomic mass of 66.58 amu, has 2 naturally occurring isotopes, ⁶⁵X (65.0457 amu, 20.53%) and ⁶⁷X (66.9704 amu, 79.47%).
What is the average atomic mass?The average atomic mass (atomic mass) of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance.
Element X has 2 isotopes:
⁶⁵X with an isotopic mass of 65.0457 amu and an abundance of 20.53% (0.2053).⁶⁷X with an isotopic mass of 66.9704 amu and an abundance of 79.47% (0.7947).We can calculate the average atomic mass of X using the following expression.
mX = m⁶⁵X × ab⁶⁵X + m⁶⁷X × ab⁶⁷X
mX = 65.0457 amu × 0.2053 + 66.9704 amu × 0.7947
mX = 66.58 amu
Element X, with an atomic mass of 66.58 amu, has 2 naturally occurring isotopes, ⁶⁵X (65.0457 amu, 20.53%) and ⁶⁷X (66.9704 amu, 79.47%).
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Nitrogen can exist as a solid, a liquid, or a gas. Which of the following lists the
phases of nitrogen in order of increasing density?
1. liquid, gas, solid
2. gas, liquid, solid
3. gas, solid, liquid
4. solid, liquid, gas
The phases of nitrogen in order of increasing density is solid, liquid, and gas.
Nitrogen is known to be odorless and colorless. Nitrogen makes up about 78% of the gases that we've in the atmosphere. It has an atomic number of 7 and is represented with the symbol N.It should be noted that nitrogen can be a solid, a liquid or a gas. When nitrogen is at ordinary pressure, it is known to be a gas. In a case whereby nitrogen is below 77°K, then it's a liquid and it's a solid when it's below 63°K.The density explains the mass per unit volume that nitrogen has when it's either at gaseous, solid or liquid state. It should be noted that the highest density is at its gaseous state.Therefore, the phases of nitrogen in order of increasing density will then be solid, liquid, and gas.In conclusion, the correct option is D.
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Answer:
Batteries hold chemical energy
Explanation:
The battery acid in a battery leads to chemical energy.
Identify the most acidic hydrogens in each of the following molecules. Give the structure of the enolate ion arising from deprotonation. (a) Acetaldehyde; (b) propanal; (c) acetone; (d) 4-heptanone; (e) cyclopentanone.
Answer:
See explanation below (Brainlist please)
Explanation:
First of all, we need to understand what is an acidic hydrogen.
An acidic hydrogen, is the atom of hydrogen which is more propense to undergo an acid base reaction, and form a stable ion or molecule in the process.
In other words, is the hydrogen that is more vulnerable to get substracted in an acid base reaction to form another compound.
Knowing this information, gives us an idea of how a molecule can be formed and which kind of compound is formed.
Now, in this question, we have 5 molecules. Each of them is either a ketone or aldehyde, so this mean that we have the carbonile group (C = O), which means that is easier to identify the acidic hydrogen. This is because the Carbonile group is an attractor group, so, it will attract the charges by inductive effect (in some cases by resonance), and the molecule is more stable.
This can be shown by drawing the enolate ion that is formed once the molecule undergo the acid base reaction. As it's an enolate form that we are looking for, then it means that the ketone or aldehyde is undergoing an electrofilic attack with a base. This base will substract the most acidic hydrogen to form a better and stable enolate. The acidic hydrogen and the enolate form can be seen in the attached picture.
a) In the case of acetaldehyde, the most acidic will be the hydrogen of carbon 2, because the hydrogen from the carbonile, once it's substracted, the charge of the carbon cannot be stabilized by resonance. Carbon 2 hydrogens, can do this job easily.
b) Propanal happens something similar to acetaldehyde, the terminal hydrogen cannot be substracted, and carbon 3, once the hydrogen is gone, the negative charge cannot be stabilized by resonance, so hydrogens of carbon 2 can do this.
c) in the case of acetone, is easier to look because we only have the C = O between two methyl group, so you can use either carbon 1 or 3 to do the job.
d) 4 heptanone the most acidic hydrogen would be carbon 3 or 5, because they are closer to the C=O and the ion can be stabilized by resonance.
e) Finally in ciclopentanone, the most acidic hydrogen would be carbon 2 or 5.
See picture for a better understanding.
Hope it helps.