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satela [25.4K]
4 years ago
10

What happens when chlorine atom gains an electron in its outer energy shell?

Chemistry
2 answers:
vfiekz [6]4 years ago
7 0
A neutrally charged chlorine atom becomes a negatively charged chlorine ion.
il63 [147K]4 years ago
3 0

Explanation:

Atomic number of chlorine is 17 and its electronic configuration is as follows.

                  1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}

Since, to become stable in nature chlorine requires only one electron from a donor atom.

As it is known that species that gain electrons will obtain a negative charge and species that lose electrons will obtain a positive charge.

Hence, when chlorine will gain an electron to become stabilized then it will change into chlorine ion or Cl^{-} ion.

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In molecular oxygen (O=O) which atom is partially positive?
saveliy_v [14]

the oxygen atom

Explanation:

Water is a molecular compound consisting of polar molecules that have a bent shape. The oxygen atom acquires a partial negative charge while the hydrogen atom acquires a partial positive charge.

4 0
4 years ago
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How are mass and weight alike?
joja [24]
Both mass and weight are measured by using scales.
7 0
3 years ago
Q Q 3. (08.02 MC)
AnnyKZ [126]

Answer: A volume of 455 mL from 0.550 M KBr solution can be made from 100.0 mL of 2.50 M KBr.

Explanation:

Given: V_{1} = ?,         M_{1} = 0.55 M

V_{2} = 100.0 mL,        M_{2} = 2.50 M

Formula used to calculate the volume of KBr is as follows.

M_{1}V_{1} = M_{2}V_{2}

Substitute the values into above formula as follows.

M_{1}V_{1} = M_{2}V_{2}\\0.55 M \times V_{1} = 2.50 M \times 100.0 mL\\V_{1} = 455 mL

Thus, we can conclude that a volume of 455 mL from 0.550 M KBr solution can be made from 100.0 mL of 2.50 M KBr.

7 0
3 years ago
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Calculate the molar mass of a gas
spin [16.1K]

Answer:

MOLAR MASS = 32 g/mol

Explanation:

Condition of standard temperature and pressure(STP) are as follow:

Temperature = 273 K

Pressure = 1 atm (or 100000 Pa)

Here atm is atmosphere and Pa is Pascal

STP conditions arte used for measuring gas density and volume using Ideal Gas Law.Here 1 mole of ideal gas occupies 22.4 L of volume.

According toi Ideal Gas Equation :

PV = nRT

where P = pressure, n= number of moles, V = volume ,R= Ideal Gas Constant and T= temperature

n=\frac{PV}{RT}

From question:

V=280 ml = 0.28 L

P = 1 atm

R=0.08205 L atm/K mol

T=273 K

Putting values in above formula :

n=\frac{1\times .280}{0.08205\times 273}

n = 0.0125 moles

Now n=\frac{given\ mass}{Molar\ mass}

Molar\ mass=\frac{given\ mass}{n}

given mass = 0.4 g (given)

Molar\ mass=\frac{0.4}{0.0125}

On solving we get:

Molar mass = 32 g/mol

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4 years ago
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I’m pretty sure it’s a
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3 years ago
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