Chemistry Fundamentals Quiz

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Questions and Answers

What is the primary characteristic that defines matter?

It consists solely of elements.

It has mass and takes up space. (correct)

It is always a solid form.

It can be created or destroyed.

Which statement correctly describes a physical change?

It alters the composition of the matter.

It never involves changes in physical states.

It results in the formation of new substances.

The composition of the substance remains unchanged. (correct)

What distinguishes a compound from a mixture?

A compound has a definite composition. (correct)

A compound can be separated by physical means.

A mixture is composed of only one kind of atom.

A compound's composition is variable.

According to Dalton's Atomic Theory, what happens to atoms in a chemical reaction?

Atoms combine to form new compounds, but are not changed. Signup and view all the answers

What identifies a diatomic molecule?

It comprises exactly two atoms. Signup and view all the answers

How are valence electrons best described?

Electrons that determine the chemical properties of an element. Signup and view all the answers

Which of the following is an example of a chemical change?

Burning paper. Signup and view all the answers

What is a characteristic of a homogeneous mixture?

It is uniformly mixed throughout. Signup and view all the answers

What characterizes an ion?

An atom that has gained or lost electrons Signup and view all the answers

Which type of bond forms between a metal ion and a nonmetal ion?

Ionic bond Signup and view all the answers

Which statement correctly describes a covalent bond?

It involves sharing electrons between nonmetals. Signup and view all the answers

What is a defining feature of nonpolar covalent compounds?

They share electrons equally. Signup and view all the answers

What happens when polar and nonpolar compounds are mixed?

They will not mix at all. Signup and view all the answers

What is required for metallic bonding?

Pooling of electrons amongst metal atoms Signup and view all the answers

What principle does the Law of Conservation of Mass state?

The total mass remains the same before and after a chemical operation. Signup and view all the answers

Which of the following is true about polar covalent compounds?

They can conduct electrical currents. Signup and view all the answers

What are reactants in a chemical reaction?

Substances that are destroyed by the reaction Signup and view all the answers

Which symbol indicates that a substance is in an aqueous solution?

(aq) Signup and view all the answers

What happens during a chemical reaction?

Bonds break and new bonds form Signup and view all the answers

Which of the following is evidence of a chemical reaction?

Formation of a gas Signup and view all the answers

What is the purpose of coefficients in a skeleton equation?

To balance the reaction Signup and view all the answers

Which of the following represents the product of the reaction Iron (s) + Chlorine (g)?

FeCl3(s) Signup and view all the answers

Which of the following is true about a skeleton equation?

It uses chemical formulas to identify substances Signup and view all the answers

What does the arrow (→) in a chemical equation signify?

The yield of products Signup and view all the answers

What does the conservation of mass state during a chemical reaction?

Atoms are neither created nor destroyed. Signup and view all the answers

Which of the following correctly represents the reaction of hydrogen and oxygen to form water?

2H2 + O2 → 2H2O Signup and view all the answers

What is the basic unit of chemical amount in the international system of units?

Mole Signup and view all the answers

In a combustion reaction, what does the substance combine with?

Oxygen Signup and view all the answers

Which type of chemical reaction involves a metal replacing a metal ion in a compound?

Single Displacement Signup and view all the answers

What is represented by the coefficients in a balanced chemical equation?

Number of molecules or moles Signup and view all the answers

What type of reaction occurs when two or more substances combine to form one substance?

Combination/Synthesis Signup and view all the answers

How many particles are in one mole of a substance?

6.022 x 10^23 Signup and view all the answers

What is the mass of unreacted KClO3 after the reaction in the experiment?

5.8 g Signup and view all the answers

According to the law of definite proportions, what remains fixed in a compound regardless of its source?

Proportions by mass of the elements Signup and view all the answers

In the formation of tin tetrabromide (SnBr4), what determines the % of tin in the compound?

Grams of Sn reacted compared to grams of SnBr4 formed Signup and view all the answers

What is the calculated mass of bromine reacted when 4.5236 g of tin reacts to form SnBr4?

0.3721 g Signup and view all the answers

Which of the following statements best describes the law of definite proportions?

The element ratios in a compound are invariant. Signup and view all the answers

When calculating the mass of unreacted KClO3, which equation accurately represents the relationship?

mass of KClO3 = mass of KCl + mass of O2 + mass of unreacted KClO3 Signup and view all the answers

What percentage of mass does hydrogen make up in water, under the law of definite proportions?

11.1% Signup and view all the answers

What do we find when we combine mass data of Sn and SnBr4 formations?

Constant proportions of tin in SnBr4 Signup and view all the answers

What is the molar mass of 1 mole of Na atom?

22.99 g/mol Signup and view all the answers

How many moles are in a 1.56 x 10^-2 g sample of juglone (C10H6O3)?

8.96 x 10^-5 mol Signup and view all the answers

Which formula correctly gives the mass percent of an element in a compound?

% Composition = (Mass of element/Molar mass of compound) x 100 Signup and view all the answers

What is the molar mass of the H2O molecule?

18.016 g/mol Signup and view all the answers

How many molecules are present in 3 moles of KCl?

1.80 x 10^24 molecules Signup and view all the answers

What is the molar mass of methane (CH4)?

16.04 g/mol Signup and view all the answers

What is the molecular formula of aspirin?

C9H8O4 Signup and view all the answers

To find the number of atoms in a given mass of an element, which relationship is used?

Mass of element = Number of moles x Molar mass Signup and view all the answers

Study Notes

Course Information

Course title: Pharmaceutical Analytical Chemistry-I
Course code: PharmD Clinical (PC101)
Academic year: 2024/2025
Instructor: Dr. Nahla Abdelshafi
Lectures: 1 & 2
Subject: General and Physical Chemistry

Course Grading

Practical exam: 20 marks
Practical exam 1 (week 7): 20 marks
Practical exam 2 (week 10): 20 marks
Evaluation: 5 marks
Periodical quizzes: 15 marks, 3 quizzes (Q1 - week 4, Q2 - week 8, Q3 - week 10, with varying marks)
Final exam: 50 marks
Oral exam: 10 marks

Course Timeline

General and Physical Chemistry: 2 lectures
Acid-base titration (aqueous + non-aqueous): 5 lectures
Precipitation: 3 lectures
Kinetics of reaction: 1 lecture

Course Regulations

Attendance: Lectures begin sharply on time. Entry is prohibited after 15 minutes. Exceeding 25% of absences may lead to penalties.
Mobile phones: Must be turned off.
Photography: Forbidden.
Audio recordings: Forbidden.

Course Outline

Chemistry: Focuses on molecules, their shape, structure and reactivity.
Weekly Schedule: A table outlining the specific lectures and quizzes for the semester.

Introduction

Chemistry: Study of matter, properties and changes.
Analytical Chemistry: Characterizing matter's composition quantitatively (how much) and qualitatively (what's present).
Matter: Anything with mass and takes up space.
Substance: Definite composition and properties (e.g. water, silver).

Classification of Matter

Substances: Can be elements or compounds.
Elements: Made of only one type of atom (e.g. carbon). Atoms are the smallest unit of an element.
Compounds: Made of two or more elements combined in a fixed ratio (e.g. water).
Mixtures: Two or more substances not chemically bonded.
- Heterogeneous: Different components easily distinguishable.
- Homogeneous: Components mixed evenly, impossible to distinguish.

Element vs. Compound

Displays diagrams of elements and compounds (e.g. H₂, O₂, N₂, Cl₂, H₂O, NO, NO₂, CO₂).

Mixtures

Mixtures: Made up of two or more substances. Not always with the same amount of each substance.
Heterogeneous: Different components easily distinguishable.
Homogeneous: Different components mixed uniformly and impossible to distinguish (e.g., solution.)

Physical and Chemical changes

Physical Change: Physical properties might change but the composition remains the same (e.g. melting ice).
Chemical Change: One or more substances are transformed into new substances with different compositions (e.g. burning paper).

Atomic Theory of Matter

Atom: Smallest particle of an element that can enter into a reaction.
Dalton's Atomic Theory: elements are composed of atoms, same elements have same properties and compounds are formed when atoms combine.

Molecules (Compounds)

Molecules: Multiple atoms joined by chemical forces.
- Diatomic: Molecules containing 2 atoms (e.g. H₂, N₂).
- Polyatomic: Molecules containing 3 or more atoms (e.g. H₂O, NH₃).
Valence Electrons: Outer shell electrons involved in bonding.

Electron Dot Diagrams (Lewis Diagrams)

Diagrams showing outer level electrons of elements.

Model of the Atom—Structure

Parts of an atom (protons, neutrons, electrons).
Atom structure—nucleus containing protons and neutrons, and electrons orbit around the nucleus.

Components of the atom

Ion: Atom or group of atoms with a net charge
Cation: Positive ion (loses electrons).
Anion: Negative ion (gains electrons).

How atoms bond

Different types of bonding: Gain electron, lose electron, pooling electrons, sharing electrons.

Ionic Bonds

Chemical bonding of oppositely charged ions.
Between a metal and nonmetal atoms.
Due to electrostatic attraction between the ions.

Covalent Bonds

Chemical bonding involving sharing electrons.
Between nonmetal atoms.
Produces molecular compounds.

Covalent Bonds—Polar vs. Nonpolar

Nonpolar compounds share electrons equally.
Polar compounds share electrons unequally.

Metallic Bonding

Chemical bonding of metal atoms.
Electrons are free to move among atoms.
Metals are good conductors, malleable, and ductile due to their bonding.

Law of Conservation of Mass

In chemical reactions, mass is neither created nor destroyed but transformed.
Total mass of reactants equals total mass of products.

Law of Definite Proportions

In a compound, the elements combine in a definite mass ratio.
Composition is fixed irrespective of the sample's source.

Chemical Reactions

Chemical reaction: One or more substances react to produce one or more new substances.
Reactants: Substances that undergo changes.
Products: Substances formed from the reaction.

Evidence for Chemical Reactions

Indicators of reactions—light/heat evolved, temperature change, gas formation, color change, precipitate formation.

Translating Word Equations to Skeleton Equations

Skeleton equations present chemical reactions using formulas, not words.

The Mole

Mole: International unit for amount of substance.
Number of particles in 1 mole = Avogadro's Number (6.022 x 10²³).
Molar mass: Mass of 1 mole of substance (grams per mole).

Composition of Compounds

Mass percentage of an element in a compound is calculated based on molar mass.

Types of Chemical Reactions

Combination/synthesis, Decomposition, Single displacement, Double displacement, Combustion.

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Description

Test your understanding of basic chemistry concepts with this quiz covering topics such as matter, chemical changes, atomic theory, and bonding. Each question will challenge your knowledge about elements, compounds, and mixtures, providing a comprehensive review of essential chemistry principles.