CHM 001

Property of a substance that remains constant during a phase change

Heat of fusion

Measure not related to a substance's ability to store thermal energy

Enthalpy change

Property that remains constant during a phase change at constant pressure

Heat of fusion

Heat required to change the temperature of one mole of a substance by 1 degree Celsius

Molar heat capacity

Property describing heat needed to convert one mole of a substance from solid to liquid

Heat of fusion

Factor determining the specific heat capacity of a substance

Chemical composition

Property representing heat needed to convert one mole of a substance from liquid to vapor

Heat of vaporization

Approximate specific heat capacity of water

4 J/g°C

Property representing heat absorbed or released during a phase change at constant temperature

Enthalpy change

Formula for calculating osmotic pressure of a solution

π = iRT

Representation of 'π' in the osmotic pressure formula

Osmotic pressure

Meaning of 'R' in the osmotic pressure formula

Ideal gas constant

Factor not part of the osmotic pressure formula

Volume (V)

Representation of 'M' in the osmotic pressure formula

Molarity of the solution

Law the osmotic pressure formula is based on

Van't Hoff's law

Effect of temperature increase on osmotic pressure of a solution

Increases

Typical unit for osmotic pressure

All of the above

Factor accounting for the presence of ions in osmotic pressure formula

i (van't Hoff factor)

Property not a colligative property

Density

Relationship between freezing point depression and solute particles concentration

Directly proportional

Property not affected by addition of a nonvolatile solute

Density

Meaning of "colligative property" in chemistry

Properties depending on solute particles concentration

Factor not affecting the extent of freezing point depression

Temperature of the solution

Practical significance of freezing point depression

Helps in determining purity of substances

Solution exhibiting the greatest freezing point depression

0.2 M NaCl solution

Property not typically used to characterize colligative properties

Volume of the solution

Factor determining osmotic pressure of a solution

Number of solute particles

Solute type contributing most to osmotic pressure

Strong electrolyte

Property measuring solution's tendency to flow through a semipermeable membrane

Osmotic pressure

Effect of temperature increase on osmotic pressure

Increases

Effect of van't Hoff factor (i) on osmotic pressure

Higher i leads to higher osmotic pressure

Solution type with highest osmotic pressure per mole

Ionic solution

Role of concentration in osmotic pressure

Higher concentration leads to higher osmotic pressure

Effect of solute addition on osmotic pressure

Increases

Phenomenon when solution's boiling point is higher than pure solvent

Boiling point elevation

Effect of solute particles number on boiling point elevation

More particles lead to greater elevation

Property affected by boiling point elevation

Vapor pressure

Relationship between boiling point elevation and solute concentration

Directly proportional

Practical application of boiling point elevation in cooking

Reduces cooking time for certain foods

Solution showing greatest boiling point elevation

Strong electrolyte solution

Meaning of van't Hoff factor (i) in boiling point elevation

Change in boiling point per mole of solute

Contribution of boiling point elevation to antifreeze effectiveness

Prevents overheating of the engine

Factor not affecting boiling point elevation

Volume of the solution

Effect of increasing pressure on gas solubility in a liquid

Increases solubility

Common unit for expressing molarity

mol/L

Common unit for volume in molarity calculation

Liters (L)

Definition of colligative property

Property dependent on solute particles concentration

Relationship between freezing point depression and solute particles presence

Directly proportional

Factor increasing solute dissolution rate in a solvent

Increasing temperature

Solvent type where non-polar solute like oil dissolves readily

Non-polar

Gas pollutant forming carboxyhemoglobin in the bloodstream

CO (Carbon Monoxide)

Bond formed when atoms transfer electrons for stability

Ionic bond

Ionic bond

A bond formed by the electrostatic attraction between positively and negatively charged ions.

Atom

The fundamental unit of an element that cannot be further broken down without changing its chemical properties.

Protons and neutrons

Particles primarily found within the nucleus of an atom.

Atomic number

The number of protons in the nucleus of an atom, corresponding to the element.

0

The electrical charge characterizing a neutron.

5

The number of valence electrons in an atom of phosphorus (P).

Oxygen (O)

The element exhibiting the highest electronegativity.

1s² 2s² 2p³

The electron configuration representing the ground state of nitrogen (N).

Cation

An atom typically transforms into a cation by losing electrons.

13

The number of electrons in a neutral atom of aluminum (Al).

Beryllium (Be)

The element exhibiting the highest ionization energy.

15

An element with 7 protons and 8 neutrons has an atomic number of 15.

+1

The charge on the resulting ion when an atom of sodium (Na) loses one electron.

Strontium (Sr)

The element with the largest atomic radius.

Valence electrons

The electrons in the outermost shell of an atom.

CH4

Among the given molecules, CH4 exhibits a nonpolar covalent bond.

Tetrahedral

The shape of a methane molecule (CH4).

109.5°

The approximate bond angle in a water (H2O) molecule.

4:5

The stoichiometric ratio of NH3 to O2 in the reaction 4NH3 + 5O2 → 4NO + 6H2O.

3 moles

If 2 moles of aluminum (Al) react with excess chlorine gas (Cl2) to produce 2AlCl3.

Gases generally have lower specific heats than liquids

A correct statement about specific heat.

Temperature

The specific heat of a substance can change with alterations in temperature.

Joules per mole

How the specific heat of a substance is typically expressed.

Helium gas

Among the listed options, the substance typically having the lowest specific heat.

Solid

The state where the specific heat of a substance is usually higher.

Decreases solubility

The effect of decreasing temperature on the solubility of most solid solutes in a liquid solvent.

It provides a direct relationship between moles of solute and volume of solution

An advantage of using molarity to express concentration.

Molarity remains constant

How molarity is affected if the volume of the solution is doubled while keeping the amount of solute constant.

Boiling point

The property of a solution affected by the addition of a nonvolatile solute.

Pressure

A factor that does NOT affect freezing point depression.

Solubility remains constant

How the solubility of a solute changes when a solution is saturated.

One vibration per second

What one Hertz represents in terms of frequency.

0.000000001 meters

One nanometer (nm) is equivalent to this length.

Lower resistance leads to higher current flow

How electric resistance is related to the flow of electric current in a conductor.

Nitrogen

The most abundant gas in the Earth's atmosphere by volume.

Increasing surface area

An action that can enhance the process of dissolution by exposing more solute to the solvent.

Non-polar

The type of solvent generally compatible with non-polar substances like hydrocarbons.

CO (Carbon Monoxide)

An air pollutant that binds strongly to hemoglobin, leading to decreased oxygen levels in the blood.

Covalent bond

The bond resulting from the electrostatic attraction between positively and negatively charged ions.

Niels Bohr

The scientist who introduced the concept of electrons orbiting the nucleus in distinct energy levels.

Protons and neutrons

What forms the central core of an atom.

Protons

The subatomic particle whose count determines the atomic number of an element.

0

The charge of a neutron.

6

An atom of oxygen (O) has six valence electrons.

Fluorine (F)

Among the listed elements, the one possessing the highest electronegativity.

1s² 2s² 2p⁶ 3s² 3p⁴

The electron configuration of sulfur (S).

Losing electrons

The transformation leading to the formation of a c

Specific Heat

The amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius.