Ask question

Ask question

All categories

3 years ago

14

Consider four atoms from the second period: lithium, beryllium boron carbon and nitrogen which of these element has the lowest e

lectronegativity value?

2 answers:

LiRa [457]3 years ago

6 0

Answer is: lithium.

Electronegativity (χ) is a property that describes the tendency of an atom to attract a shared pair of electrons.

Electronegativity increases from left to right across a period.

Atoms with higher electronegativity attracts more electrons towards it, electrons are closer to that atom.

For example nitrogen has electronegativity approximately χ = 3 and lithium has χ = 1, so if they form bond, nitrogen will have negative and lithium positive charge.

bearhunter [10]3 years ago

5 0

Lithium has the lowest. if fluorine is the highest then lithium is the lowest. i hope this helps you out!

You might be interested in

A flexed bow has __________ energy. The energy is due to its ____________. When the string is released, work will be done to the

Phoenix [80]

Answer:

its not c or d because we know nothing will happen to the bow- so its up to a and b- making the answer b :V

Explanation:

3 0

3 years ago

. Which of the following statement is not related to a chemical reaction ? A. New substances are formed B. Atoms of the elements

kodGreya [7K]

Answer:

the answer should be B because elements do not tranform into other elements in a chemical reaction

am I right please?

5 0

3 years ago

A 18.08-g sample of the ionic compound , where is the anion of a weak acid, was dissolved in enough water to make 116.0 mL of so

Oksi-84 [34.3K]

Answer:

a) 129.14 g/mol

b) 8.87

Explanation:

Given that:

mass of the ionic compound [NaA] = 18.08 g

Volume of water = 116.0 mL = 0.116 L

Let the mole of the acid HCl = 0.140 M

Volume of the acid = 500.0 mL = 0.500 L

pH = 4.63

$V_{equivalence}_{acid}$ = 1.00 L

Equation for the reaction can be represented as:

$NaA_{(aq)} + HCl_{(aq)} -----> HA_{(aq)} + NaCl_{(aq)$

From above; 1 mole of an ionic compound reacts with 1 mole of an acid to reach equivalence point = 0.140 M × 1.00 L

= 0.140 mol

Thus, 0.140 mol of HCl neutralize 0.140 mol of ionic compound at equilibrium

Thus, the molar mass of the sample = $\frac{18.08g}{0.140 mole}$

= 129.14 g/mol

b) since pH = pKa

Then pKa of HA = 4.63

Ka = $10^{-4.63]$

= $2.3*10^{-5}$

$[A^-]equ = \frac{0.140M*1.00L}{1.00L+0.116L}$

$= \frac{0.140 mol}{1.116 L}$

= 0.1255 M

$K_a$ of HA = $2.3*10^{-5}$

$K_b = \frac{1.0*10^{-14}}{2.3*10^{-5}}$

$= 4.35*10^{-10}$

$A_{(aq)}$ + $H_2O_{(l)}$ $\rightleftharpoons$ $HA_{(aq)}$ + $OH^-_{(aq)}$

Initial 0.1255 0 0

Change - x + x + x

Equilibrium 0.1255 - x x x

$K_b = \frac{[HA][OH^-]}{[A^-]}$

$4.35*10^{-10} = \frac{[x][x]}{[0.1255-x]}$

As $K_b$ is very small, (o.1255 - x) = 0.1255

$x = \sqrt{0.1255*4.35*10^{-10}}$

[OH⁻] = $x = 7.4 *10^{-6}$

But pOH = - log [OH⁻]

= - log [ $7.4*10^{-6}$ ]

= 5.13

pH = 14.00 = 5.13

pH = 8.87

6 0

3 years ago

Dinitrogen monoxide gas is collected at 19.0 °C in an evacuated flask with a measured volume of 30.0 L. When all the gas has bee

torisob [31]

Answer:

The mass of dinitrogen monoxide gas that is collected is 27.6 grams

Explanation:

<u>Step 1:</u> Data given

Molar mass of N2O = 44.013 g/mole

Temperature = 19.0 °C = 292 Kelvin

volume of the gas = 30.0 L

Pressure of the gas = 0.500 atm

Gasconstant = 0.08206 L*atm/K*mol

<u>Step 2</u>: Calculate number of moles

via the ideal gas law:

P*V = n*R*T

n= (P*V)/(R*T)

n= (0.500 atm * 30.0 L)/(0.08206 L*atm/K*mol *292 K)

n =0.626

<u>Step 3:</u> Calculate mass of dinitrogen monoxide

mass = number of moles * Molar mass

mass of N2O = 0.626 moles * 44.013 g/mole

mass of N2O = 27.6 grams

The mass of dinitrogen monoxide gas that is collected is 27.6 grams

8 0

3 years ago

Have a definite volume, but move quickly enough to overcome the forces of attraction

patriot [66]

Answer:

do you have a pic

Explanation:

6 0

3 years ago

Read 2 more answers