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3 years ago

explain how a metal with one valence electron compares with a metal with more than one valence electron

Chemistry

1 answer:

slamgirl [31]3 years ago

7 0

Explanation:

A metal with one valence electron is highly reactive compared to those with more than one electron.

Atoms including those of metals reacts in order attain a stable electronic configuration just like those of noble gases.

An atom with one valence electron have just one electron in its valence shell.

Metals generally have large sizes.
when the electron in this shell is lost, the metal atom can then attain stability.
therefore, such atom will quickly want to combine with any other willing to accept the electron so that they can be stable.
Those with more than one electron will find it difficult to lose them.
It requires huge energy to remove such electrons compared to the ones with only one valence electron.

learn more:

Valence electrons brainly.com/question/3023499

#learnwithBrainly

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Calculate the molarity (M) if 3.35g of H3PO4 is dissolved in water to give a total volume of 200mL

lyudmila [28]

Answer:

0.171 M

Explanation:

Step 1: Given data

Mass of H₃PO₄ (solute): 3.35 g

Volume of solution (V): 200 mL

Step 2: Calculate the moles of solute

The molar mass of H₃PO₄ is 97.99 g/mol.

3.35 g × 1 mol/97.99 g = 0.0342 mol

Step 3: Convert "V" to liters

We will use the conversion factor 1 L = 1000 mL.

200 mL × 1 L/1000 mL = 0.200 L

Step 4: Calculate the molarity of the solution

We will use the definition of molarity.

M = moles of solute / liters of solution

M = 0.0342 mol/0.200 L = 0.171 M

8 0

3 years ago

How many grams are in 4.3 x 10 -4 moles of calcium phosphate?

attashe74 [19]

Explanation:

Ca3(PO4)2 1 mole has 310.2 g

Ca3(PO4)2 4.3 × 10^-4 moles has 4.3 × 10^-4 × 310.2

= 1,333.86 × 10^-4

= 1.334 × 10^-1

OR 0.1334 g

5 0

3 years ago

The specific heat of gold is 0.126 J/gºC. How much energy is released

Schach [20]

Explanation:

Specific heat capacity of gold (S)

= 0.126 J /kg°C

mass (m) = 350 g = 0.35 kg

difference in temperature (dt)

= 88.5°C - 24.6°C

= 63.9° C

Now

Energy released (Q)

= m*s*dt

= 0.35 * 0.126 * 63.9

= 2.81799 Joule

Hope it will help :)

3 0

3 years ago

Which of the following contains BOTH ionic and covalent bonds? Which of the following contains BOTH ionic and covalent bonds? Ca

Marta_Voda [28]

Answer:

BaSO₄

Explanation:

It is possible to know if a bond is ionic or covalent using the electronegativity of the atoms in the bond. If electronegativity difference is higher than 1.8, the bond is ionic, if doesn't, bond is covalent.

CaI₂ has the Ca-I bond where electronegativity of Ca and I are 1 and 2.66. Difference of electronegativity is 1.66 → Bond is covalent.

COS has the C-O and C-S bonds where electronegativity of C, O and S are 2.55, 3.44 and 2.55. Difference of electronegativity are 0.89 and 0 → Bonds are covalent.

BaSO₄ has the Ba-O and O-S bonds where electronegativity of Ba, O and S are 0.89, 3.44 and 2.55. Difference of electronegativity are 2.55 and 0.89 → Bonds are ionic and covalent respectively.

SF₆ has the S-F bond where electronegativity of S and F are 2.55 and 3.98. Difference of electronegativity is 1.43 → Bond is covalent.

4 0

4 years ago

Compared to a solution with a ph of 6, the hydronium ion concentration of a solution with a Ph of 4 has how many more times the

Alexxx [7]

Answer: The hydronium ion concentration of a solution with a pH of 4 is 100 times more than the the hydronium ion concentration of a solution with a pH of 6

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

$pH=-\log [H^+]$

1. Solution with pH of 6

$6=-\log [H^+]$

$[H^+]=10^{-6}$

2. Solution with pH of 4

$4=-\log [H^+]$

$[H^+]=10^{-4}$

$\frac{H^+_4}{H^+_6}=\frac{10^{-4}}{10^{-6}}=10^{2}={100}$

${H^+_4}=100\times {H^+_6}$

Thus the hydronium ion concentration of a solution with a pH of 4 is 100 times more than the the hydronium ion concentration of a solution with a pH of 6

5 0

3 years ago