chem rev term 2 Flashcards
(28 cards)
According to the Kinetic Molecular Theory, which statement is TRUE about gas particles?
They have constant random motion.
Gas particles move freely and collide with each other and the walls of their container.
What is the SI unit for pressure?
Pascal (Pa).
Other units for pressure include atmospheres (atm) and millimeters of mercury (mmHg).
Which tool is commonly used to measure atmospheric pressure?
Barometer.
A barometer measures the pressure exerted by the atmosphere.
According to Dalton’s Law of Partial Pressures, the total pressure of a mixture of gases is:
The sum of the partial pressures of each gas.
This law allows for the calculation of the total pressure in a gas mixture.
In Graham’s Law, the rate of effusion of a gas is:
Inversely proportional to the square root of its molar mass.
This means lighter gases effuse faster than heavier gases.
What happens to gas particles during diffusion?
They spread randomly from high to low concentration.
Diffusion is driven by the concentration gradient.
When forming ionic bonds, metals tend to:
Lose electrons.
Metals become positively charged cations by losing electrons.
What is the primary cause of gas pressure?
Particle collisions with container walls.
Pressure is a result of the frequency and force of collisions between gas particles and the walls of their container.
Which statement about effusion is correct?
Lighter gases effuse faster than heavier gases.
Effusion rates are affected by the molar mass of the gases.
In ionic compound formation, what type of ions do non-metals typically form?
Negative ions.
Non-metals gain electrons to achieve a full valence shell.
The Kinetic Molecular Theory explains all of the following EXCEPT:
Chemical reactions between gases.
The theory primarily deals with gas behavior, not chemical reactions.
Which unit conversion is correct?
1 atm = 760 mmHg.
This conversion is commonly used in pressure calculations.
What factor affects the rate of gas diffusion?
The molar mass of the gas.
Lighter gases diffuse faster than heavier gases due to lower molar mass.
In an ionic bond, the attraction is between:
Oppositely charged ions.
Ionic bonds form between cations and anions.
According to Graham’s Law, if gas A effuses twice as fast as gas B, what is the relationship between their molar masses?
Mass of B is four times mass of A.
The relationship is derived from the inverse square root of their molar masses.
What happens to gas pressure when temperature increases at constant volume?
Pressure increases.
Increased temperature leads to increased kinetic energy of gas particles, resulting in higher pressure.
In the formation of an ionic compound between sodium and chlorine, what occurs?
Sodium loses an electron and chlorine gains an electron.
This transfer of electrons leads to the formation of Na⁺ and Cl⁻ ions.
When gas A diffuses twice as slowly as gas B, what can you conclude?
Gas A has four times the molar mass of gas B.
This conclusion is based on Graham’s Law of Diffusion.
In a covalent bond, what happens to the electrons between atoms?
Electrons are shared between atoms.
Covalent bonds involve the sharing of electron pairs between atoms.
What type of elements typically form covalent bonds with each other?
Nonmetals with nonmetals.
Covalent bonds usually occur between nonmetal elements.
According to Graham’s Law, helium diffuses about _______ times faster than carbon dioxide.
3.32.
This is based on the molar masses of helium and carbon dioxide.
The scenario of perfume spreading in a room demonstrates:
Diffusion.
Gas particles move from high to low concentration areas.
Higher temperature means _______ kinetic energy for gas particles.
Higher.
Increased temperature increases the speed of gas particles.
To determine the relative molar masses of gases using diffusion rates, apply:
Graham’s Law of Diffusion.
This law states that the rate of diffusion is inversely proportional to the square root of the molar mass.
