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Questions and Answers
What type of mixture is formed when sugar is dissolved in water?
What type of mixture is formed when sugar is dissolved in water?
Which process can separate a compound into its elements?
Which process can separate a compound into its elements?
In a solution, the substance that is present in the largest amount is known as the:
In a solution, the substance that is present in the largest amount is known as the:
Which of the following is an example of a heterogeneous mixture?
Which of the following is an example of a heterogeneous mixture?
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What distinguishes the properties of compounds from their individual elements?
What distinguishes the properties of compounds from their individual elements?
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What defines isotopes of a given element?
What defines isotopes of a given element?
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Which term describes a neutral atom that loses electrons?
Which term describes a neutral atom that loses electrons?
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What is a molecule?
What is a molecule?
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What distinguishes a homonuclear molecule from a heteronuclear molecule?
What distinguishes a homonuclear molecule from a heteronuclear molecule?
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What is the temperature in Kelvin when given a temperature of 28 °C?
What is the temperature in Kelvin when given a temperature of 28 °C?
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Which formula represents the actual number and types of atoms in a molecule?
Which formula represents the actual number and types of atoms in a molecule?
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What is the temperature in Celsius for a child with a temperature of 104 °F?
What is the temperature in Celsius for a child with a temperature of 104 °F?
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How is the empirical formula related to the molecular formula?
How is the empirical formula related to the molecular formula?
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If the temperature is 300 K, what is it in Fahrenheit?
If the temperature is 300 K, what is it in Fahrenheit?
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Which example represents a heteronuclear molecule?
Which example represents a heteronuclear molecule?
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What happens to sodium (Na) when it loses one electron?
What happens to sodium (Na) when it loses one electron?
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How many milliliters are in 1 cubic meter (m³)?
How many milliliters are in 1 cubic meter (m³)?
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What is the density of a substance if its mass is 3.4 kg and volume is 0.25 L?
What is the density of a substance if its mass is 3.4 kg and volume is 0.25 L?
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What is the relationship between mass and volume for calculating density?
What is the relationship between mass and volume for calculating density?
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What is the derivation of the SI unit for density?
What is the derivation of the SI unit for density?
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How many cubic centimeters are in 1 nanoliter (nL)?
How many cubic centimeters are in 1 nanoliter (nL)?
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What characteristic is true for solids?
What characteristic is true for solids?
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What type of matter cannot be separated into simpler substances by chemical means?
What type of matter cannot be separated into simpler substances by chemical means?
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Which separation method is used for mixtures?
Which separation method is used for mixtures?
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What describes a gas's behavior in a container?
What describes a gas's behavior in a container?
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A homogeneous mixture is characterized by which of the following?
A homogeneous mixture is characterized by which of the following?
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What is the empirical formula for C6H12O6?
What is the empirical formula for C6H12O6?
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Which of the following compounds has a structural formula that indicates the attachment of atoms?
Which of the following compounds has a structural formula that indicates the attachment of atoms?
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Which formula represents the simplest form of C6H14?
Which formula represents the simplest form of C6H14?
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What does the molecular formula represent?
What does the molecular formula represent?
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What is the building unit of a compound?
What is the building unit of a compound?
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Which statement describes metals in the context of ionic compounds?
Which statement describes metals in the context of ionic compounds?
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In the periodic table, what are the vertical columns called?
In the periodic table, what are the vertical columns called?
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Which of these compounds is an example of an ionic compound?
Which of these compounds is an example of an ionic compound?
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How many significant figures are in the measurement 100041 m?
How many significant figures are in the measurement 100041 m?
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What will be the result of rounding 3.679 to three significant figures?
What will be the result of rounding 3.679 to three significant figures?
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If you multiply 1.4 by 8.011 and divide by 5.12, how many significant figures should the final answer have?
If you multiply 1.4 by 8.011 and divide by 5.12, how many significant figures should the final answer have?
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When rounding the number 12.4997 to five significant figures, what is the correct result?
When rounding the number 12.4997 to five significant figures, what is the correct result?
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Which of the following numbers has the least significant figures?
Which of the following numbers has the least significant figures?
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What is the result of rounding 3.305 to three significant figures?
What is the result of rounding 3.305 to three significant figures?
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How many significant figures are in the number 0.0050700 km?
How many significant figures are in the number 0.0050700 km?
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Study Notes
Introduction to Matter
- Chemistry is the study of matter and the changes it undergoes.
- Matter is anything that has mass and occupies space (volume).
- Matter is composed of particles.
States of Matter
- Solid: Particles are closely packed in an orderly arrangement. Particles have little freedom of motion. Solids have a fixed volume and shape.
- Liquid: Particles are close together but not rigidly held in position. Particles can move past each other. Liquids have a fixed volume but take the shape of the container they fill.
- Gas: Particles are randomly spread apart. Particles have complete freedom of movement. Gases assume both the shape and volume of their container.
Classification of Matter
- Matter can be classified as a pure substance or a mixture.
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Pure substances can be elements or compounds.
- Elements cannot be broken down into simpler substances by chemical means (e.g., iron, mercury, oxygen).
- Compounds are formed when two or more elements chemically combine in definite ratios (e.g., salt, water, ethane, carbon dioxide). The properties of compounds are different from the properties of the elements they are made from.
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Mixtures are a physical combination of two or more pure substances.
- Homogeneous mixtures have a uniform composition throughout (e.g., sugar dissolved in water, air, sea water). A homogeneous mixture of two or more substances is called a solution. The solute is the substance present in the smallest amount and the solvent in the largest amount.
- Heterogeneous mixtures have a non-uniform composition (e.g., sugar mixed with iron filings, sand and chalk powder).
Mixtures Continued
- Filtration: a physical method used to separate heterogeneous solid-liquid mixtures (e.g., mixture of water and sand)
- Distillation: a physical method used to separate a homogenous solid-liquid mixture (e.g., salt water).
Properties of Matter
- Chemical properties: describe a substance's ability to change into a new substance(s) (e.g., heat of combustion, enthalpy of formation, electronegativity)
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Physical properties: can be observed or measured without changing the substance's composition (e.g., temperature, color, volume, mass, area, pressure, melting point, boiling point).
- Intensive Properties: do not depend on the amount of matter (e.g., temperature, density, boiling point, concentration, solubility, color).
- Extensive Properties: depend on the amount of matter (e.g., mass, volume, surface area, amount of substance).
Changes in Matter
- Chemical Change: Involves making or breaking chemical bonds, resulting in the formation of new substances. (e.g., oxidation-reduction, reaction of an acid and base, heat decomposition, electrolysis of water, iron rusting, combustion of ethane, burning of wood)
- Physical Change: Alters a substance's physical form but does not change its chemical identity. (e.g., phase changes - vaporization, condensation, freezing, sublimation, melting, deposition; dissolving sugar and salts; mixing sand with water)
Physical Quantities and SI Units
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Fundamental Quantities: cannot be defined in terms of other physical quantities.
- Length (meter)
- Mass (kilogram)
- Temperature (Kelvin)
- Time (second)
- Amount of substance (mole)
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Derived Quantities: can be defined in terms of fundamental quantities.
- Volume (m³)
- Density ( kg/m³)
- concentration
- Pressure (Pascal)
SI Prefixes
- Used to express very large or very small quantities (e.g., tera, giga, mega, kilo, deci, centi, milli, micro, nano, pico).
Density
- Density is an intensive property that describes the mass per unit volume of a substance.
- SI unit is kg/m³ (g/cm³ also common)
Solubility
- Solubility: the maximum amount of a solute that will dissolve in a given amount of solvent at a given temperature.
- Depends on the temperature.
Significant Figures
- Used to express the uncertainty of measured results.
- Non-zero digits are significant.
- Zeros between non-zero digits are significant.
- Zeros to the left of the first non-zero digit are NOT significant.
- Zeros to the right of the last non-zero digit are significant IF a decimal point is present.
Uncertainty in Measurement
- Measurement is comparing an unknown quantity to a known one.
- Exact numbers are obtained from defined values (counts, conversion factors).
- Inexact numbers (measured values) have uncertainty (e.g. the last digit is an estimate)
Uncertainty in Calculations
- When adding or subtracting, the result is rounded to the least precise decimal position, not the least significant digit.
- When multiplying or dividing, the answer has the same number of significant figures as the measurement with the least number of significant figures.
Accuracy vs Precision
- Accuracy: how close a measurement is to the true or accepted value.
- Precision: how close repeated measurements are to each other.
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Description
Explore the fundamental concepts of matter in this introductory quiz on chemistry. Learn about the different states of matter, their characteristics, and how matter is classified into pure substances and mixtures. Perfect for students beginning their chemistry studies.
