Chemistry Lab and Nuclear Chemistry Review

Flashcards covering general lab safety, measurements, states of matter, basic atomic structure, periodic trends, and nuclear chemistry concepts from lecture notes.

What are the main safety procedures in the chemistry lab?

Wear goggles, follow instructions, handle chemicals carefully, know emergency equipment, and dispose of waste properly.

Name three common lab equipment items and their uses.

Beaker (holding liquids), graduated cylinder (measuring volume), balance (measuring mass).

What is the difference between base and scientific notation?

Base notation is standard numbers (e.g., 3,000), while scientific notation expresses numbers with a power of ten (e.g., 3.0 
×
10³).

What are the metric units of length, mass, volume, and temperature?

Length: meter (m); Mass: gram (g); Volume: liter (L); Temperature: Celsius (°C). Prefixes (kilo, centi, milli, etc.) show multiples or fractions of base units.

Define significant figures.

The digits in a measurement that represent known precision plus one estimated digit.

How do you round answers with significant figures?

Match the result to the least precise measurement in the calculation.

What is dimensional analysis?

A method that uses conversion factors and unit cancellation to solve problems.

What are examples of conversion factors used in chemistry problems?

Metric equalities (1 km = 1000 m), percentages (25% = 25/100), given rates (60 miles/hour), changing units within a problem.

Define volume, mass, and density.

Volume = space occupied (L, mL, cm³), Mass = matter amount (g), Density = Mass/Volume (g/mL or g/cm³).

How can density be used in calculations?

Density can be used as a conversion factor (e.g., g 
→
mL or mL 
→
g).

How is matter classified?

Pure substances (elements, compounds) and mixtures (homogeneous, heterogeneous).

What are the three main states of matter and their characteristics?

Solid: fixed shape/volume; Liquid: fixed volume, variable shape; Gas: variable shape/volume.

Define kinetic and potential energy with examples.

Kinetic = energy of motion (moving car); Potential = stored energy (chemical bonds, a rock on a hill).

What are the energy units and their relationships?

calorie (cal), dietary Calorie (1 Cal = 1000 cal), joule (J), kilojoule (kJ).

How do you convert between °F and °C?

°C = (°F 
−
32) 
×
5/9; °F = (°C 
×
9/5) + 32.

How do you convert between °C and K?

K = °C + 273; °C = K 
−
273.

What is absolute zero in Celsius and Kelvin?

-273 °C and 0 K.

What is the formula for heat calculations?

Q = mass 
×
specific heat 
×
∆T. Can solve for Q, mass, SH, or ∆T.

Define specific heat.

Amount of heat needed to raise 1 g of a substance by 1 °C.

What is the specific heat of water?

1 cal/g°C, which defines the calorie.

Define element, compound, and atom.

Element: pure substance of one atom type; Compound: 2+ elements bonded; Atom: smallest unit of matter.

How do you use the periodic table to find element groups and families?

Groups/families = columns; Periods = rows; Alkali metals = group 1; Halogens = group 17; Noble gases = group 18; Metals on left, non-metals on right, metalloids on staircase.

What are the charges and relative masses of subatomic particles?

Proton: +1, 1 amu; Neutron: 0, 1 amu; Electron: 
−1
, ~0 amu.

Define atomic number.

Number of protons; also equals electrons in a neutral atom.

Define mass number.

Sum of protons + neutrons in nucleus.

How do you calculate protons, neutrons, and electrons from atomic and mass numbers?

Protons = atomic number; Neutrons = mass number 
−
atomic number; Electrons = protons (in neutral atom).

Define isotope.

Atoms of same element with different neutrons (different mass number).

What is the Octet Rule?

Atoms gain/lose/share electrons to achieve 8 valence electrons in outer shell.

What periodic trends should be recognized?

Atomic size: increases down group, decreases across period; Ionization energy: decreases down group, increases across period; Metallic character: increases down group, decreases across period.

What are the four types of radiation?

Alpha (
α
), Beta (
β
), Positron (
β
■), Gamma (
γ
).

What are the biological effects of radiation?

Can damage cells, DNA, cause mutations, increase cancer risk.

How do you write balanced nuclear decay equations?

Show both mass number and atomic number balanced on both sides (e.g., 
α
decay: ²³■U 
→
²³■Th + 
α
).

What is the formula for half-life problems?

Remaining = Initial 
×
(½)■, where n = time elapsed 
÷
half-life.

What are some applications of radioactivity?

Medical imaging, cancer treatment, carbon dating, nuclear power.

What is the difference between nuclear fission and fusion?

Fission: splitting heavy nuclei (used in reactors); Fusion: combining light nuclei (powers the sun).