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3 years ago

Which best describes the electron behavior in metallic bonding?

Chemistry

1 answer:

aliya0001 [1]3 years ago

4 0

They are delocalized.

When you think of a bond, you probably think of the "ball and stick" model of bonding where there are two atoms connected by one or more bonds. The bonds between those two atoms connect only those two atoms. Because the bond just stays put, it's referred to as localized covalent bonding.

However, metals do different stuff. If you've got a metal, you've got a great big bunch of atoms all held together in a great big bunch of valence electrons. Rather than two valence electrons forming a single bond between two metal atoms, you have all of the valence electrons from every atom in the element moving around all over the place in delocalized bonds. If you imagine putting a bunch of pieces of Velcro into a pile of yarn, the electrons are represented by the disordered yarn and the metal atoms are represented by the Velcro.

OK.

Got for - M<span>isterguch</span>

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4Fe + 302 → 2Fe2O3

frez [133]

Answer:

2 -> O and Fe

Explanation:

5 0

3 years ago

Consider the following system at equilibrium where \Delta H° = 18.8 kJ, and Kc = 9.52×10-2, at 350 K.

slega [8]

Answer:

1. C. remains the same. 2. C. is less than Kc. 3. B. run in the reverse direction to reestablish equilibrium. 4. A. increase.

Explanation:

At constant temperature, the equilibrium concentration has not effect on the equilibrium constant because the rate constants do not change with change in the concentrations or amounts of the reactants or products. Change in the concentration of one reactant or product causes the concentration of the others to change so as to maintain a constant value for the equilibrium constant. On the other hand, the reaction quotient is used to measure the relative amounts of reactants and products during a chemical reaction at any point in time. The value of the reaction quotient shows the direction of the chemical reaction.

Therefore, when 0.31 moles of CCl4(g) are removed from the equilibrium system at constant temperature:

1. the value of Kc remains the same

2. the value of Qc is less than Kc

3. the reaction must run in the reverse direction to reestablish equilibrium

4. the concentration of $CH_{4}$ will increase because product will be converted to reactants to reestablish equilibrium.

7 0

3 years ago

Which is not a waste product of cellular respiration heat oxygen carbon dioxide or water?

horsena [70]

Carbon Dioxide is used in celular respiration. All other choices are waste products

7 0

3 years ago

What do organisms have based on their functions?

mote1985 [20]

Unicellular organisms, cells perform all the basic actions and functions required for living like nutrition, respiration, reproduction etc.

In multicellular organisms, cells divide their tasks on the basis of "DIVISION OF LABOUR" to specialize in certain functions besides respiration etc. Like conduction in neurons, excitation in muscles, RBC production by bone marrow etc.

6 0

3 years ago

What is the molar mass of a gas if a flask with a volume of 3. 16 l contains 9. 33 grams of the gas at 32. 0°c and 1. 00 atm?

Serhud [2]

The molar mass of a gas if a flask with a volume of 3. 16 L contains 9. 33 grams of the gas at 32. 0°C and 1. 00 atm is 1.17g/mol

Calculation ,

In this question we have to fist find the number of moles of gas by using ideal gas equation and from the help of number of moles we can determine molar mass.

According to ideal gas equation which is also known as ideal law ,

PV = nRT ...( i )

where P is the pressure of the gas = 1 atm

V is the volume of the gas in the flask with volume = 3. 16 L

R is the universal gas constant = 0.082 atm L/K mol

T is the temperature = 32. 0°C = 32 + 273 = 305 K

n is the number of moles = ?

Putting the value of Pressure P , volume V , temperature T , number of moles n and universal gas constant R in the equation (i) we get ,

1 atm ×3. 16 L = n× 0.082 atm L/K mol ×305 K

n = 1 atm ×3. 16 L / 0.082 atm L/K mol × 305 K = 0.126 mole

number of mole of a gas = 0.126 mole = given mass/ molar mass

molar mass = number of moles × Given mass = 0.126 × 9. 33 = 1.17g/mol

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1 year ago