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Questions and Answers
According to the Particle Model of Matter, what primarily differentiates solids, liquids, and gases?
According to the Particle Model of Matter, what primarily differentiates solids, liquids, and gases?
- The type of atoms present in each state.
- The amount of energy and space between particles, and their movement. (correct)
- The external pressure applied to each state.
- The color of the substance in each state.
A molecule is always composed of different types of atoms.
A molecule is always composed of different types of atoms.
False (B)
Explain how particles in a solid differ from those in a gas regarding energy and movement.
Explain how particles in a solid differ from those in a gas regarding energy and movement.
Particles in a solid have less energy and movement compared to particles in a gas. Solid particles vibrate in fixed positions, while gas particles move freely and rapidly.
A ________ is a pure substance that cannot be broken down into simpler substances by chemical means, whereas a ________ is a substance composed of two or more elements chemically bonded together.
A ________ is a pure substance that cannot be broken down into simpler substances by chemical means, whereas a ________ is a substance composed of two or more elements chemically bonded together.
Which of the following is a key difference between a homogeneous and heterogeneous mixture?
Which of the following is a key difference between a homogeneous and heterogeneous mixture?
Match each substance with its correct classification:
Match each substance with its correct classification:
A physical change results in the formation of a new substance, whereas a chemical change only alters the state or appearance of the existing substance.
A physical change results in the formation of a new substance, whereas a chemical change only alters the state or appearance of the existing substance.
Which observation is LEAST likely to indicate that a chemical reaction has taken place?
Which observation is LEAST likely to indicate that a chemical reaction has taken place?
Explain the difference between a physical property and a chemical property of a substance, and provide an example of each.
Explain the difference between a physical property and a chemical property of a substance, and provide an example of each.
A scientific ________ describes what nature does under certain conditions, while a scientific ________ explains why nature behaves in that way.
A scientific ________ describes what nature does under certain conditions, while a scientific ________ explains why nature behaves in that way.
Which feature is characteristic of Thomson’s “Plum Pudding” atomic model?
Which feature is characteristic of Thomson’s “Plum Pudding” atomic model?
The atomic number of an element represents the total number of protons and neutrons in the nucleus of an atom of that element.
The atomic number of an element represents the total number of protons and neutrons in the nucleus of an atom of that element.
Explain how an atom of fluorine differs from a fluoride ion ($F^-$).
Explain how an atom of fluorine differs from a fluoride ion ($F^-$).
________ is credited with developing the first periodic table, which was significant because it organized elements based on their properties and predicted the existence of undiscovered elements.
________ is credited with developing the first periodic table, which was significant because it organized elements based on their properties and predicted the existence of undiscovered elements.
Which group of elements is known for being the MOST reactive?
Which group of elements is known for being the MOST reactive?
Match the following properties to the correct group of elements:
Match the following properties to the correct group of elements:
For the compound $Fe_2O_3$ (s), what elements are present, how many atoms of each element are present, and what is its state of matter?
For the compound $Fe_2O_3$ (s), what elements are present, how many atoms of each element are present, and what is its state of matter?
Ionic compounds involve the sharing of electrons between atoms, whereas molecular compounds involve the transfer of electrons.
Ionic compounds involve the sharing of electrons between atoms, whereas molecular compounds involve the transfer of electrons.
How are molecular compounds named differently than ionic compounds? Give an example.
How are molecular compounds named differently than ionic compounds? Give an example.
In the chemical equation $2H_2 + O_2
ightarrow 2H_2O$, $H_2$ and $O_2$ are the ________ and $H_2O$ is the ________.
In the chemical equation $2H_2 + O_2 ightarrow 2H_2O$, $H_2$ and $O_2$ are the ________ and $H_2O$ is the ________.
Flashcards
Particle Model of Matter: 5 Points
Particle Model of Matter: 5 Points
Matter is made of tiny particles, particles are always moving, particles have space between them, increasing temperature increases particle motion, and particles attract each other.
Solid vs. Gas (Particle Model)
Solid vs. Gas (Particle Model)
Solids: Low energy, little space, vibrate in place. Gases: High energy, large space, move freely.
Mixture vs. Pure Substance
Mixture vs. Pure Substance
Mixtures are combinations of substances; pure substances are not. Example: Mixture - Salad; Pure substance - Gold
Pure Substance vs. Pure Element
Pure Substance vs. Pure Element
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Homogeneous vs. Heterogeneous Mixture
Homogeneous vs. Heterogeneous Mixture
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Physical vs. Chemical Change
Physical vs. Chemical Change
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Evidence of Chemical Reaction
Evidence of Chemical Reaction
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Law vs. Theory
Law vs. Theory
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Atomic Model Characteristics
Atomic Model Characteristics
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What is an Element?
What is an Element?
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Atomic Number vs. Atomic Mass
Atomic Number vs. Atomic Mass
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Most/Least Reactive Elements
Most/Least Reactive Elements
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Metals vs. Non-metals vs. Metalloids
Metals vs. Non-metals vs. Metalloids
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Ionic vs. Molecular Compounds
Ionic vs. Molecular Compounds
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Naming: Molecular vs. Ionic
Naming: Molecular vs. Ionic
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Reactants vs. Products
Reactants vs. Products
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Endothermic vs. Exothermic
Endothermic vs. Exothermic
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Types of Chemical Reactions
Types of Chemical Reactions
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Speeding Up Reaction Rate
Speeding Up Reaction Rate
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Catalyst
Catalyst
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Study Notes
- These notes refer to matter and chemical changes
Particle Model of Matter
- Atoms are the basic building blocks of matter
- Elements are substances made of only one type of atom
- Molecules are formed when two or more atoms are chemically bonded
Five Main Points of the Particle Model of Matter
- All matter is made up of tiny particles
- Particles are in constant motion
- Particles have space between them
- Particles are attracted to one another
- Particles move faster when heated
States of Matter
- Energy: Gas particles have more energy than solid particles
- Space: Gas particles have more space between them than solid particles
- Movement: Gas particles move more freely than solid particles
Pure Substances vs. Mixtures
- Pure substances consist of only one type of particle (e.g., distilled water)
- Mixtures consist of two or more types of particles (e.g., air)
Pure Substances vs. Pure Elements
- A pure substance can be an element or a compound
- A pure element consists of only one type of atom (e.g., gold)
- A compound consists of two or more types of atoms chemically bonded together (e.g., water)
Homogeneous vs. Heterogeneous Mixtures
- Homogeneous mixtures (solutions) have uniform composition throughout (e.g., salt water)
- Heterogeneous mixtures (mechanical mixtures) have non-uniform composition (e.g., salad)
Classification of Substances
- Distilled water: Pure substance
- Granite: Mechanical mixture
- Apple juice: Solution
Physical vs. Chemical Change
- Physical Change:
- What changes? The form or appearance of the substance
- New substance formed? No
- Reversible? Often
- Examples: Melting ice, boiling water
- Chemical Change:
- What changes? The chemical composition of the substance
- New substance formed? Yes
- Reversible? Rarely
- Examples: Burning wood, rusting iron
Evidence of Chemical Reactions
- Change in color
- Change in odor
- Formation of a precipitate (solid)
- Formation of a gas (bubbles)
- Release or absorption of heat (change in temperature)
- Emission of light
Physical vs. Chemical Properties
- Reacts with oxygen: Chemical
- Highly malleable: Physical
- Not soluble in water: Physical
- pH of 4.0: Chemical
- Conducts electricity: Physical
- Yellow in color: Physical
- Extremely toxic: Chemical
- Low density: Physical
Laws vs. Theories
- A law is a descriptive statement about a phenomenon based on repeated observations (e.g., law of conservation of mass)
- A theory is an explanatory statement about a phenomenon, based on evidence and reasoning (e.g., atomic theory)
Atomic Models
- Thomson’s “Plum Pudding” Model:
- Electrons are scattered throughout a positively charged sphere
- Rutherford’s “Planetary” Model:
- A central positive nucleus is orbited by electrons
- Bohr’s Atomic Model:
- Electrons orbit the nucleus in specific energy levels
- Electron Cloud Model:
- Electrons exist in probability clouds (orbitals) around the nucleus
Elements
- An element is a substance made of only one type of atom (e.g., hydrogen)
Components of an Atom
- Proton: Positively charged particle in the nucleus
- Neutron: Neutral particle in the nucleus
- Electron: Negatively charged particle orbiting the nucleus
Atomic Number vs. Atomic Mass
- The atomic number is the number of protons in an atom of an element
- The atomic mass is the average mass of an atom of an element
- Atomic number identifies the element
- In a neutral atom, the number of protons equals the number of electrons
Fluorine Atom
- A neutral fluorine atom has 9 protons and 9 electrons
Fluorine Ion
- A fluoride ion with a charge of -1 has 9 protons and 10 electrons
Development of the Periodic Table
- Dmitri Mendeleev is credited with developing the first periodic table
- It was a great achievement because he arranged elements by increasing atomic mass and grouped them by similar properties
Periodic Table Trends
- The most reactive group of elements is the alkali metals (Group 1)
- The least reactive group of elements is the noble gases (Group 18)
Properties of Metals, Non-Metals, and Metalloids
- Metals:
- State at room temp.: Solid (except mercury)
- Appearance: Shiny, silvery
- Conductivity: High
- Malleability and ductility: Malleable and ductile
- Non-Metals:
- State at room temp.: Solid, liquid, or gas
- Appearance: Dull
- Conductivity: Low
- Malleability and ductility: Brittle
- Metalloids:
- State at room temp.: Solid
- Appearance: Can be shiny or dull
- Conductivity: Intermediate
- Malleability and ductility: Brittle
Chemical Formulas
- H2O (g): Hydrogen and oxygen; 2 hydrogen atoms, 1 oxygen atom; gas
- CO2 (g): Carbon and oxygen; 1 carbon atom, 2 oxygen atoms; gas
- Fe2O3 (s): Iron and oxygen; 2 iron atoms, 3 oxygen atoms; solid
- HCl (l): Hydrogen and chlorine; 1 hydrogen atom, 1 chlorine atom; liquid
Ionic vs. Molecular Compounds
- Ionic compounds are formed through ionic bonds between metals and non-metals
- Molecular compounds are formed through covalent bonds between non-metals
Ionic vs. Molecular - Identification
- NH3: Molecular
- H2O2: Molecular
- SO2: Molecular
- ZnSO2: Ionic
- NaBr: Ionic
- K2S: Ionic
- NO: Molecular
- H2O: Molecular
Naming Compounds
- Molecular compounds use prefixes to indicate the number of atoms of each element
- Ionic compounds do not use prefixes, and the metal name stays the same while the non-metal name ends in "-ide"
Naming and Formulas of Compounds
- Carbon tetrachloride: CCl4
- KCl: Potassium chloride
- Nitrogen monoxide: NO
- SiO2: Silicon dioxide
- Ag2S: Silver sulfide
- Sodium sulfide: Na2S
- C4H10: Tetracarbon decahydride (Butane)
- CuO: Copper (II) oxide
- AgNO3: Silver nitrate
- Iron (II) oxide: FeO
- N2O5: Dinitrogen pentoxide
- Lithium oxide: Li2O
- Calcium chloride: CaCl2
Chemical Equations
- Word equation: Solid silver reacts with liquid bromine to produce solid silver bromide
- Chemical equation: 2Ag(s) + Br2(l) → 2AgBr(s)
Reactants vs. Products
- Reactants are the starting materials in a chemical reaction
- Products are the substances formed as a result of a chemical reaction
Endothermic vs. Exothermic Reactions
- Endothermic reactions absorb heat from the surroundings, causing a decrease in temperature (e.g., melting ice)
- Exothermic reactions release heat to the surroundings, causing an increase in temperature (e.g., burning wood)
Beaker Cooling Down
- If a beaker cools down when two chemicals are combined, the reaction is endothermic
- This is because the reaction is absorbing heat from the surroundings (the beaker)
Types of Chemical Reactions
- Formation:
- Definition: Two or more reactants combine to form one product
- Example: 2H2 + O2 → 2H2O
- Decomposition:
- Definition: One reactant breaks down into two or more products
- Example: 2H2O → 2H2 + O2
- Single Replacement:
- Definition: One element replaces another element in a compound
- Example: Zn + 2HCl → ZnCl2 + H2
- Double Replacement:
- Definition: Two compounds exchange ions or elements
- Example: AgNO3 + NaCl → AgCl + NaNO3
- Combustion:
- Definition: A rapid reaction between a substance and oxygen, producing heat and light
- Example: CH4 + 2O2 → CO2 + 2H2O
Classifying Chemical Reactions
- C12H22O11 + O2 → CO2 + H2O: Combustion
- Fe + O2 → Fe2O3: Formation
- Mg3(PO4)2 + H2 → Mg + H3PO4: Single Replacement
- Al2S3 → Al + S: Decomposition
Factors Affecting Reaction Rates
- Increase the temperature
- Increase the concentration of reactants
- Increase the surface area of solid reactants
- Add a catalyst
Catalysts
- A catalyst is a substance that speeds up a chemical reaction without being consumed in the reaction
- Catalysts lower the activation energy of a reaction, making it easier for the reaction to occur
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