Chemistry Chapter 1 Quiz

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Questions and Answers

What is a characteristic of a gas?

Atoms are fluid and take on the shape of their container. (correct)

Atoms are evenly distributed without any space between them.

Atoms are in a solid structure that vibrates in place.

Atoms are tightly packed in a fixed arrangement.

Which of the following best describes a heterogeneous mixture?

A combination that appears blended yet retains distinct components. (correct)

A solution completely dissolved in a solvent.

Composed of only one type of substance.

The same uniform composition throughout.

What is the correct formula for density?

D = V/m

D = m/V (correct)

D = M/V

D = m × V

What type of change is sublimation?

A transition from solid to gas without becoming a liquid. Signup and view all the answers

Which of the following statements about significant figures is true?

In multiplication, the result should have the same number of significant figures as the factor with the least. Signup and view all the answers

How is the standard deviation calculated?

S = √(∑(X−X̄)²/(n-1)) Signup and view all the answers

Which statement best describes a qualitative measurement?

It focuses on the physical properties or appearance of a substance. Signup and view all the answers

What does the ionic charge indicate?

The net charge resulting from the loss or gain of electrons. Signup and view all the answers

Identify the limiting reactant in the reaction given the provided moles of reactants.

B2 Signup and view all the answers

What is the hybridization and molecular geometry of a molecule with four bonding domains and no nonbonding domains?

sp3, Tetrahedral Signup and view all the answers

Calculate the moles of NH₄Br produced from 0.0313 mol of Br₂ based on the molar ratio from the reaction.

0.0626 mol Signup and view all the answers

What is the calculated mass of NH₄Br produced when using 0.0626 mol?

6.13 g Signup and view all the answers

What is the correct balanced chemical equation for the reaction involving A₂ and B₂ producing AB₂?

2A2 + 6B2 → 4AB2 Signup and view all the answers

What is the percentage yield if the actual yield of a reaction producing 4.71 g of product from 6.13 g theoretical yield?

76.8% Signup and view all the answers

What is the molar mass of ammonia (NH₃)?

17.0 g/mol Signup and view all the answers

Which configuration describes the 4s subshell?

n=4, l=0, m_l=0, m_s=+1/2 Signup and view all the answers

What is the correct order of ionic compounds based on Coulombic attraction?

MgO < KF < NaF Signup and view all the answers

Which statement accurately describes ionization energy trends across groups?

Group 15 elements have higher ionization energy than Group 16 due to electron pairing. Signup and view all the answers

According to Graham's Law, which scenario is correctly stated?

Rate(A) / Rate(B) = √(M_B / M_A) Signup and view all the answers

What would be the molarity of a solution if its pH is 3?

Molarity = 10^-3 Signup and view all the answers

In the context of the periodic table, which property generally increases from left to right?

Ionization energy Signup and view all the answers

Which electron configuration represents the Plumbic ion (Pb⁺⁴)?

[Xe] 6s² 4f¹⁴ 5d⁰ 6p⁴ Signup and view all the answers

Which scenario correctly describes Bohr's theory limitations?

It is only applicable to hydrogen and cannot handle more complex atoms. Signup and view all the answers

Study Notes

Law vs. Theory

Laws describe a body of facts, while theories explain a body of facts.

States of Matter

Solids: Atoms are in a fixed shape, vibrating.
Liquids: Atoms take shape, more hitting.
Gases: Atoms all over, most space.

Homogenous vs Heterogenous Mixtures

Homogenous: Solution (e.g., steel, milk)
Heterogenous: Mixture (e.g., blood, brass)

Separation Methods

Filtration: Coffee filter
Distillation: Heating flask
Chromatography: Ink separation
Electrolysis: Compounds into elements (e.g., H₂O)

Density

Density (D) = mass (m) / volume (V) or V = m/D or m = D x V

Extensive vs Intensive Properties

Extensive properties depend on the amount of substance (e.g., mass, volume, heat).
Intensive properties do not depend on the amount of substance (e.g., melting point, boiling point, density).

Physical vs Chemical Changes

Physical change: Alterations in a substance's physical properties (e.g., melting, boiling).
Chemical change: Alterations that create new substances by rearranging atoms (e.g., reactions, burning).

Kinetic vs Potential Energy

Kinetic Energy: Energy of motion (e.g., thermal, mechanical, electrical, acoustic).
Potential Energy: Stored energy of position or status (e.g., gravitational, electrostatic, chemical, nuclear).

Law of Conservation of Energy

Endothermic: Absorbs heat
Exothermic: Emits heat

Qualitative vs Quantitative

Qualitative: Physical appearance or feel.
Quantitative: Numbers or units.

Temperature Conversions

°C + 273.15 = K
K - 273.15 = °C

Precision vs Accuracy

Precision: How close measurements are to each other.
Accuracy: How close measurements are to the true value.

Relative Error

Relative error = (observed value - accepted value) / accepted value x 100%

Percentage Yield

% yield = (actual yield / theoretical yield) x 100%

Significant Figures (Sig Figs)

Rules for addition/subtraction: Least significant decimal place after the decimal point
Rules for multiplication/division: Least significant figure present

Scientific Discoveries

Rutherford: Atomic nucleus
Millikan: Electron charge
Thomson: Charge/mass ratio of electron
Dalton: Atomic weight
Becquerel/Curie: Radiation (radioactivity)

Atomic/Mass/lonic Numbers

Atomic number (# of protons)
Mass number (# of protons + neutrons)
lonic charge: Ions
Protons → lonic charge
Proton + Neutrons

Isotopes

Atoms of the same element with different numbers of neutrons
(relative abundance) x (atomic mass) / 100.
Sum it to find X

Periodic Table Trends

Electronegativity increases across a period and decreases down a group, reflecting the tendency to gain electrons
Ionic compounds: Metal + nonmetal, roman numerals.

Covalent Compounds

Nonmetal + nonmetal (prefixes: mono, di, tri, tetra, penta, hexa, hepta, octa, and nona,deca).

Oxidation States

Oxidation state: The charge an atom would have if all bonds were ionic.
Free elements have an oxidation state of 0.
Fluorine is always -1.
Oxygen is usually -2.
Group 1: +1, Group 2: +2, Group 3: +3.
Hydrogen is usually +1; with nonmetals, +1; with metals, -1

Oxidation-Reduction (Redox) Reactions

Oxidation: Loss of electrons
Reduction: Gain of electrons
Oxidizing agent: Substance causing oxidation
Reducing agent: Substance causing reduction

Acid-Base Reactions

Acids react with bases to produce water and a salt.
H₂SO₄ + NaOH → H₂O + Na₂SO₄.

Stoichiometry

The quantitative relationships between reactants and products in a chemical reaction (balancing).
Limiting reactant: The reactant that is completely used up first in a reaction

Molarity

Moles of solute / Liters of solution

Percent Composition

% element = ((Molar mass of element) / (Molar mass of compound)) × 100

Empirical Formula

Simplest whole-number ratio of atoms in a compound

Molecular Formula

Actual number of atoms of each element in a molecule

Gram-Molecular Mass

The mass in grams of one mole of a substance. (Molar Mass)

Mole Conversions

Moles = mass / molar mass
Moles = number of particles / Avogadro's number

Photons

E photon = hc / λ

Electromagnetic Radiation

The energy-carrying waves; radio-infrared-microwaves-visible-ultraviolet-x-rays-gamma
Wavelength-Frequency

Bohr Theory

Electron orbits around the nucleus.

Electron Configurations

Arrangement of electrons in orbitals and sublevels
Quantum numbers (n, l, ml, and ms).

Hybridisation

The concept of hybridization describes the mixing of atomic orbitals in an atom to form hybrid orbitals that participate in chemical bonding.

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Description

Test your knowledge on the fundamental concepts of chemistry with this quiz. Topics include the characteristics of gases, heterogeneous mixtures, density formulas, types of changes, significant figures, and standard deviation calculations. Perfect for students looking to reinforce their understanding of basic chemical principles.