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3 years ago

The electron configuration of nitrogen (N) is?

Chemistry

2 answers:

snow_tiger [21]3 years ago

7 0

The correct is A. 1s22s22p3

Hope it helps

Archy [21]3 years ago

5 0

Answer: The electron configuration of nitrogen (N) is 1s22s22p3.

Explanation:

When electrons of an atom are distributed in a molecular orbital then this distribution is known as electronic configuration.

Atomic number of nitrogen is 7 and its electronic distribution is 2, 5.

Whereas the electronic configuration of nitrogen is as follows.

$1s^{2}2s^{2}2p^{3}$

Thus, we can conclude that out of the given options only option (A) depicts correct electron configuration of nitrogen (N).

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explain observation made when anhydrous calcium chloride and anhydrous copper (ii) sulphate are separately exposed to the atmosp

Burka [1]

Answer:

Anhydrous calcium chloride dissolves and becomes liquid

Anhydrous copper (ii) sulphate will produce crystal particles

Explanation:

Anhydrous calcium chloride is deliquescent and hence when it is exposed to air, it absorbs water from air. After absorbing water, it dissolves and after some time a pool of clear liquid appears.

Anhydrous copper (ii) sulphate will form crystal structures and the following reaction will takes place

CuSO4 + 5 H20 --> CuSO4.5H2O

6 0

3 years ago

The freezing point of water H2O is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is urea. If 13.

Trava [24]

Answer:

Molality = 1.46 molal

The freezing point of the solution = -2.72 °C

Explanation:

Step 1: Data given

The freezing point of water H2O is 0.00°C at 1 atmosphere

urea = nonelectrolyte = van't Hoff factor = 1

Mass urea = 13.40 grams

Molar mass urea = 60.1 g/mol

Mass of water = 153.2 grams

Molar mass H2O = 18.02 g/mol

Kf = 1.86 °C/m

Step 2: Calculate moles urea

Moles urea = mass urea /molar mass urea

Moles urea = 13.40 grams / 60.1 g/mol

Moles urea = 0.223 moles

Step 3: Calculate the molality

Molality = moles urea / mass water

Molality = 0.223 moles / 0.1532 kg

Molality = 1.46 molal

Step 4: Calculate the freezing point of the solution

ΔT = i * Kf * m

ΔT = 1* 1.86 °C/m * 1.46 m

ΔT = 2.72 °C

The freezing point = -2.72 °C

3 0

3 years ago

What is the symbol (including the atomic number, mass number, and element symbol) for the nitrogen isotope with 8 neutrons? Expr

Doss [256]

Answer: The isotope is represented as $_7^{15}\textrm{N}$

Explanation:

General representation of an element is given as: $_Z^A\textrm{X}$

where,

Z represents Atomic number

A represents Mass number

X represents the symbol of an element

Atomic number is defined as the number of protons or number of electrons that are present in an atom.

Atomic number = Number of electrons = Number of protons = 7 (for nitrogen)

Mass number is defined as the sum of number of protons and neutrons that are present in an atom.

Mass number = Number of protons + Number of neutrons = 7+8 = 15

Thus the isotope is represented as $_7^{15}\textrm{N}$

5 0

3 years ago

The rate constants of some reactions double with every 10 degree rise in temperature. Assume that a reaction takes place at 271

AfilCa [17]

Answer : The activation energy for the reaction is, 119.7 J

Explanation :

According to the Arrhenius equation,

$K=A\times e^{\frac{-Ea}{RT}}$

or,

$\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$K_1$ = rate constant at 271 K

$K_2$ = rate constant at 281 K = $2K_1$

$Ea$ = activation energy for the reaction = ?

R = gas constant = 8.314 J/mole.K

$T_1$ = initial temperature = 271 K

$T_2$ = final temperature = 281 K

Now put all the given values in this formula, we get:

$\log (\frac{2K_1}{K_1})=\frac{Ea}{2.303\times 8.314J/mole.K}[\frac{1}{271K}-\frac{1}{281K}]$

$Ea=119.7J$

Therefore, the activation energy for the reaction is, 119.7 J

3 0

4 years ago

Consider the reaction below. mc009-1.jpg If the reaction is at dynamic equilibrium at 500 K, which statement applies to the give

Bas_tet [7]

The answer is ( The concentrations of the products and reactants do not change.)

6 0

3 years ago

Read 2 more answers