Answer: Electrovalent bonds are produced when electrons are transferred from atoms of one element to atoms of another element, producing positive and negative ions. The bond which is formed by the transfer of electrons between the atoms is called electrovalent bond or ionic bond. Electrovalent bonds are only formed between metals and non-metals. Electrovalent bonds are not formed between two non-metals.
In simple words electrovalent bond involves the transference of a certain number of electrons to another dissimilar atom which has a tendency to gain electrons so that both acquire stable inert gas configurations. The electrostatic attraction always tends to decrease the potential energy. Hence, the potential energy of the system is much less than it was before the formation of an ionic bond.
Explanation: An Ionic bond is the bond formed by the complete transfer of valence electron to attain stability.
This type of bonding leads to the formation of two oppositely charged ions – positive ion known as cations and negative ions are known as anions.
The presence of two oppositely charged ions results in a strong attractive force between them. This force is an ionic or electrovalent bond.
Ionic bonds form between atoms with large differences in electronegativity, whereas covalent bonds formed between atoms with smaller differences in electronegativity.
The compound formed by the electrostatic attraction of positive and negative ions is called an ionic compound.
Answer:
Explanation:
Considering:
Given :
For NaOH :
Molarity = 0.0500 M
Volume = 45.88 mL
The conversion of mL to L is shown below:
1 mL = 10⁻³ L
Thus, volume = 45.88×10⁻³ L
Moles of NaOH = Moles of monoprotic acid
So, moles of monoprotic acid = 0.002294 moles
Given that:- mass = 0.456 g
The formula for the calculation of moles is shown below:
Thus,
Answer:
1.98 g
Explanation:
The balanced reaction would be:
2CO + O2 = 2CO2
We assume that the gases are ideal gas so that we use the relation that 1 mol of an ideal gas is equal to 22.4 L of the gas at STP. From that relation, we get the number of moles and we can convert it to other units. We do as follows:
1.0 L CO ( 1 mol / 22.4 L ) ( 2 mol CO2 / 2mol CO ) = 0.045 mol CO2 produced
0.045 mol CO2 ( 22.4 L / 1 mol ) = 1 L of CO2
0.045 mol CO2 ( 44.01 g / 1 mol ) = 1.98 g of CO2
Answer: a) 211 mm Hg
b) 0.629 grams
Explanation:
According to Dalton's law, the total pressure is the sum of individual pressures.
= total pressure = 750 mmHg
= 124 mm Hg
= 218 mm Hg
= 197 mm Hg
= ?
Thus the partial pressure of the helium gas is 211 mmHg.
b) According to the ideal gas equation:
P = Pressure of the gas = 211 mmHg = 0.28 atm (760mmHg=1atm)
V= Volume of the gas = 13.0 L
T= Temperature of the gas = 282 K
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas= ?
Mass of helium= 
Thus mass of helium gas present in a 13.0-L sample of this mixture at 282 K is 0.629 grams
Answer:
Elements that occupy the same column on the periodic table
