Physical Chemistry and Halogens Quiz

Definition: The branch of chemistry that deals with the physical properties and changes of matter.
Key Concepts:
- Thermodynamics: Study of energy changes in chemical reactions; includes laws of thermodynamics.
- Kinetics: Rate of chemical reactions and factors influencing these rates.
- Equilibrium: Conditions under which the forward and reverse reactions occur at the same rate.
- Quantum Chemistry: Study of the quantum mechanical properties of atoms and molecules.
- Electrochemistry: Relation between electricity and chemical changes; involves redox reactions.

Composition: Consists of fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
Properties:
- Nonmetals, with increasing atomic number showing increasing atomic size and decreasing electronegativity.
- High reactivity, especially with alkali metals to form salts (halides).
- Exhibit diatomic molecules (e.g., F2, Cl2).
Trends:
- As you descend the group, melting and boiling points increase.
- Reactivity decreases down the group.
Uses:
- Chlorine in water purification.
- Fluorine in toothpaste for dental health.

Composition: Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).
Properties:
- Soft, highly reactive metals that can easily lose one electron to form +1 ions.
- Low melting and boiling points (decrease down the group).
- Low density, with some elements (Li, Na, K) being less dense than water.
Trends:
- Reactivity increases down the group; reactions with water become more vigorous.
- Reaction with halogens forms ionic compounds (e.g., NaCl).
Uses:
- Sodium in street lighting and chemical synthesis.
- Lithium in batteries.

Composition: Includes helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
Properties:
- Colorless, odorless, and non-toxic gases at room temperature.
- Very low reactivity due to a complete valence shell; inert.
- Monatomic gases, exhibiting weak van der Waals forces.
Trends:
- Boiling and melting points increase down the group.
- Higher atomic number correlates with increased density.
Uses:
- Neon in signs; argon in welding to create an inert atmosphere; helium in balloons.

Studies the physical properties and changes of matter
Key areas include thermodynamics, kinetics, equilibrium, quantum chemistry, and electrochemistry

Includes Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), and Astatine (At)
Nonmetals with increasing atomic size and decreasing electronegativity as you move down the group
Highly reactive, especially with alkali metals to form salts (halides)
Exist as diatomic molecules (e.g., F2, Cl2)
Melting and boiling points increase as you move down the group
Reactivity decreases down the group
Uses include chlorine for water purification and fluorine in toothpaste

Consists of Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr)
Soft, highly reactive metals that easily lose one electron to form +1 ions
Low melting and boiling points, decreasing down the group
Low density, with some (Li, Na, K) less dense than water
Reactivity increases down the group, leading to more vigorous reactions with water
React with halogens to form ionic compounds (e.g., NaCl)
Uses include sodium in street lighting and chemical synthesis, lithium in batteries

Comprises Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn)
Colorless, odorless, and non-toxic gases at room temperature
Very low reactivity due to a complete valence shell; inert
Monatomic gases exhibiting weak van der Waals forces
Boiling and melting points increase down the group
Higher atomic number correlates with increased density
Uses include neon in signs, argon in welding, and helium in balloons