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sp2606 [1]
3 years ago
5

Four atoms are arbitrarily labeled D, E, F, and G. Their electronegativities are as follows: D = 3.8, E = 3.3, F = 2.8, and G =

1.3. If the atoms of these elements form the molecules DE, DG, EG, and DF, how would you arrange these molecules in order of increasing covalent bond character? (Use the appropriate <, =, or > symbol to separate substances in the list.)
Chemistry
1 answer:
PSYCHO15rus [73]3 years ago
3 0

Answer:

Thus the order of covalent character will be

DG < EG < DF < DE

Explanation:

The electronegativity decides the nature of bond formed between two atoms.

More the difference in electronegativity more the ionic character in the bond formed.

Let us check the electronegativity difference between the elements forming molecules

a) DE :

3.8-3.3 = 0.5

b) DG :

3.8-1.3 = 2.5

c) EG

3.3-1.3 = 2

d) DF

3.8-2.8 = 1.3

So the maximum ionic character will be in DG and minimum in DE

Thus the order of covalent character will be

DG < EG < DF < DE

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Arrange the following H atom electron transitions in order of increasing frequency of the photon absorbed or emitted:
Setler [38]

The order of frequency is d < a < c < b

E_{n} = 13.6 * z^{2} / n^{2} eV

where z = atomic mass number

n = energy level

For hydrogen z = 1

Therefore, Energy for n = 1

E_{n} = 13.6 * 1^{2} / 1^{2} eV

     = -13.6 eV

for n = 2

E_{n} = 13.6 * 1^{2} / 2^{2} eV

     = -3.40 eV

for n = 3

 E_{n} = 13.6 * 1^{2} / 3^{2} eV

      = -1.51 eV

for n = 4

 E_{n} = 13.6 * 1^{2} / 4^{2} eV

      = -0.85 eV

for n = 5

 E_{n} = 13.6 * 1^{2} / 5^{2} eV

      = -0.544 eV

n = 2 to n = 4 (absorption)

ΔE = E4 - E2   = -0.85 - (-3.40) = 2.55 eV

n = 2 to n = 1 (emission)

ΔE =  E1 - E2  = -13.6 - (-3.40) = -10.2eV

The negative sign indicates that emission will take place.

n = 2 to n = 5 (absorption)

ΔE = E5 - E2 = -0.544 - (-3.40) = 2.856 eV

n = 4 to n = 3 (emission)

ΔE = E3 - E4 = -1.51 - (-0.85) = -0.66 eV

We know that

E = h * υ

Therefore, Energy is proportional to frequency.

So increasing the order of energy is

E4  < E1  < E3  <  E2

order of frequency is

d < a < c < b

For more information click on the link below:

brainly.com/question/17058029

# SPJ4

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1 year ago
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Arkeisha is correct because the fluid in an alkaline battery has a ph between 7.1 and 14.0
8 0
3 years ago
When electromagnetic radiation of wavelength 300nm falls on the surface of sodium electrons are emitted with a KE of 1.68 * 10 5
gtnhenbr [62]

Answer:

3.83 × 10⁻¹⁹ J;  518 nm  

Step-by-step explanation:

The equation for the <em>photoelectric effect</em> is

hf = Φ + KE  

<em>Data: </em>

λ = 300 nm = 300 × 10⁻⁹ m

KE = 1.68 × 10⁵ J/mol

Calculations:

Part 1. Minimum energy to remove an electron

(a) Calculate the <em>energy of the photon</em>

fλ = c  

 f = c/λ     Divide each side by λ

E = hf

E = hc/λ

E = (6.626× 10⁻³⁴ × 2.998 × 10⁸)/(300 × 10⁻⁹)

E = 6.622 × 10⁻¹⁹ J

(b) Calculate the <em>KE of one electron</em>

KE = 1.68 × 10⁵ × 1/(6.022 × 10²³)

KE = 2.790 × 10⁻¹⁹ J

(c) Calculate the work function

hf = Φ + KE     Subtract KE from each side

Φ = 6.622 × 10⁻¹⁹  - 2.790 × 10⁻¹⁹

Φ = 3.83 × 10⁻¹⁹ J

The minimum energy to remove an electron from a sodium atom

is 3.83 × 10⁻¹⁹ J.

Part 2. Maximum wavelength to remove an electron

The photon must have just enough energy to overcome the work function and leave the electron with zero kinetic energy.

    E = Φ

hc/λ = Φ                      Multiply each side by λ

  hc = Φ λ                   Divide each side by Φ

   λ = hc/ Φ

   λ = (6.626 × 10⁻³⁴ × 2.998 × 10⁸)/(3.83 × 10⁻¹⁹)

   λ = 5.18 × 10⁻⁷ m     Convert to nanometres

   λ = 518 nm

The maximum wavelength that will cause an electron to move is 518 nm.

6 0
3 years ago
Read 2 more answers
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