Particle Model of Matter Quiz

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Questions and Answers

What is true about particles in a solid compared to those in a gas?

  • Particles in solids are further apart than those in gases.
  • Particles in solids move faster than those in gases.
  • Particles in solids have less energy than those in gases. (correct)
  • Particles in solids are not attracted to one another.

Which statement differentiates a homogeneous mixture from a heterogeneous mixture?

  • Homogeneous mixtures contain multiple types of particles.
  • Homogeneous mixtures appear as one substance. (correct)
  • Heterogeneous mixtures cannot be physically separated.
  • Heterogeneous mixtures contain particles that are uniformly distributed.

Which of the following is an example of a pure substance?

  • Gold bar (correct)
  • Granite
  • Apple juice
  • Chocolate chip cookie

In what way do molecules differ from elements?

<p>Molecules can contain more than one type of atom. (D)</p> Signup and view all the answers

What characterizes a chemical change?

<p>A new substance is formed. (C)</p> Signup and view all the answers

Which of the following is a characteristic of the particle model of matter?

<p>Particles are attracted to each other regardless of their state. (C)</p> Signup and view all the answers

How is a solution defined in relation to a mechanical mixture?

<p>Solutions have components that are mixed uniformly. (B)</p> Signup and view all the answers

What distinguishes a pure substance from a pure element?

<p>A pure substance can be a compound. (A)</p> Signup and view all the answers

What type of chemical reaction is represented by the equation $2H2(g) + O2(g) → 2H2O(l)$?

<p>Formation (A)</p> Signup and view all the answers

Which of the following describes an endothermic reaction?

<p>Absorbs heat energy (B)</p> Signup and view all the answers

What product forms when silver reacts with bromine?

<p>Silver bromide (C)</p> Signup and view all the answers

Which factor would NOT speed up a chemical reaction?

<p>Decreasing surface area (A)</p> Signup and view all the answers

What is the primary difference between an exothermic and endothermic reaction?

<p>Exothermic reactions release energy, while endothermic reactions absorb energy. (D)</p> Signup and view all the answers

What type of reaction is shown by $Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)$?

<p>Single Replacement (A)</p> Signup and view all the answers

Given the reaction $NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)$, what type of reaction is it?

<p>Double Replacement (D)</p> Signup and view all the answers

Which of the following compounds is classified as ionic?

<p>AgBr (A)</p> Signup and view all the answers

What condition would increase the rate of a reaction in a beaker?

<p>Increasing the surface area of solid reactants (A)</p> Signup and view all the answers

Which of the following compounds represents a molecular compound?

<p>C4H10 (A)</p> Signup and view all the answers

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

<p>Flammability (C)</p> Signup and view all the answers

What is the main distinction between a law and a theory in scientific terms?

<p>A theory describes what happens, while a law explains why it happened. (B)</p> Signup and view all the answers

In the context of atomic models, who proposed that electrons exist in fixed pathways around the nucleus?

<p>Bohr (A)</p> Signup and view all the answers

What does the atomic number of an element indicate about a neutral atom of that element?

<p>It indicates the number of protons and electrons. (A)</p> Signup and view all the answers

Which group of elements is known to exhibit the highest reactivity?

<p>Nonmetals (B)</p> Signup and view all the answers

Which characteristic is NOT true about metals?

<p>They are usually gases at room temperature. (D)</p> Signup and view all the answers

What is the difference between ionic and molecular compounds?

<p>Ionic compounds are made up of non-metals and metals. (D)</p> Signup and view all the answers

How are molecular compounds named differently from ionic compounds?

<p>Molecular compounds use prefixes to indicate the number of atoms. (B)</p> Signup and view all the answers

What is the primary characteristic of the electron cloud model?

<p>It uses mathematical equations to predict electron locations. (B)</p> Signup and view all the answers

What type of bond typically forms in molecular compounds?

<p>Covalent bonds (A)</p> Signup and view all the answers

When considering properties of elements, which of the following are typically found in non-metals?

<p>Brittle and not ductile (C)</p> Signup and view all the answers

What is the role of the nucleus in an atom?

<p>It has a positive charge and contains protons and neutrons. (A)</p> Signup and view all the answers

What is the state of matter for the compound Fe2O3?

<p>Solid (B)</p> Signup and view all the answers

A neutral atom of fluorine differs from a fluoride ion with a -1 charge because:

<p>It has an equal number of protons and electrons. (B)</p> Signup and view all the answers

Flashcards

Particle Model of Matter

All matter is made up of tiny particles called atoms. These atoms are always moving and have spaces between them. The attraction between these particles, and how much they move, determines the state of matter (solid, liquid, gas).

What is an element?

An element is a pure substance that cannot be broken down further. It is made up of only one type of atom.

What is a molecule?

A molecule is formed when two or more atoms bond together. These atoms can be the same or different.

What is a pure substance?

A pure substance is made up of only one type of particle, either an element or a compound.

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What is a mixture?

A mixture is a combination of two or more substances that can be easily separated. Mixtures can be either homogeneous or heterogeneous.

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What is a homogeneous mixture?

A homogeneous mixture has a uniform composition throughout. Meaning it's blended so well you can't see the different parts.

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What is a heterogeneous mixture?

A heterogeneous mixture has a non-uniform composition. Different parts are easy to see.

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What is a physical change?

A physical change only changes the form or appearance of a substance, not its chemical composition.

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What is a chemical change?

A chemical change results in the formation of a new substance with different properties.

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Formation reaction

A chemical reaction where two or more reactants combine to form a single product.

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Decomposition reaction

A chemical reaction where a single compound breaks down into two or more simpler substances.

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Single replacement reaction

A chemical reaction where one element replaces another element in a compound.

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Double replacement reaction

A chemical reaction where two compounds react, and the cations and anions of the reactants swap places, forming two new compounds.

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Combustion reaction

A chemical reaction where a substance reacts with oxygen, releasing energy in the form of heat and often light.

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Endothermic reaction

A chemical reaction that absorbs heat or energy from its surroundings.

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Exothermic reaction

A chemical reaction that releases heat or energy into its surroundings.

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Catalyst

A substance that can be added to some chemical reactions to speed up the reaction rate without being consumed in the process.

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Reactants and products

The reactants are the substances that are used up in a chemical reaction. The products are the substances that are formed in a chemical reaction.

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Factors that increase reaction rate

Increasing the temperature, stirring, increasing reactant concentration, and increasing surface area.

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Chemical Change

A change where a new substance is formed with different properties.

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Physical Change

A change where the substance remains the same, only its physical properties are altered.

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Scientific Law

A description of what happens in nature, usually expressed as a mathematical equation.

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Scientific Theory

A well-substantiated explanation of some aspect of the natural world, supported by evidence.

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Scientific Model

A simplified representation of a complex system used to explain and predict phenomena.

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Atom

The smallest unit of an element that retains the chemical properties of that element.

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Proton

A positively charged particle found in the nucleus of an atom.

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Neutron

A neutral particle found in the nucleus of an atom.

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Electron

A negatively charged particle that orbits the nucleus of an atom.

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Atomic Number

The number of protons in the nucleus of an atom, which determines the element's identity.

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Atomic Mass

The total number of protons and neutrons in the nucleus of an atom.

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Element

A pure substance made up of only one type of atom. Examples: oxygen, gold, hydrogen.

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Compound

A substance formed when two or more different elements chemically combine. Examples : water, salt.

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Ionic Bond

A bond formed by the electrostatic attraction between oppositely charged ions.

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Covalent Bond

A bond formed by the sharing of electrons between atoms.

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Study Notes

Particle Model of Matter

  • All matter is composed of extremely tiny particles (atoms).
  • There are spaces between these particles.
  • Particles attract each other.
  • Particles are constantly moving.
  • Particles move faster and farther apart when energy is added.

Atom, Element, and Molecule

  • Atoms are the fundamental building blocks of all matter.
  • Elements are types of atoms.
  • Molecules are combinations of atoms.

Differences Among States of Matter

  • Solids: Particles are tightly packed, have low energy, little movement, and are close together.
  • Gases: Particles are widely spaced, have high energy, move rapidly, and are far apart.

Pure Substances, Solutions, and Mechanical Mixtures

  • Pure substance: Contains only one type of particle (e.g., gold bar, water).
  • Mixture: Contains two or more different types of particles (e.g., chocolate chip cookie, salad).
  • Solution (homogeneous mixture): Particles are uniformly distributed (e.g., wine, coffee, blood).
  • Mechanical mixture (heterogeneous mixture): Particles are not uniformly distributed (e.g., pizza, sandwich, granite).

Pure Substance vs. Pure Element

  • A pure substance can be an element or a compound.
  • A pure element is a substance composed of only one type of atom.

Physical and Chemical Changes

  • Physical change: Changes the form (e.g., shape, size, state) but not the chemical identity of a substance.
  • Chemical change: Changes the chemical composition, resulting in new substances.
PHYSICAL CHANGE CHEMICAL CHANGE
Changes in form (shape, size, state) but not its chemical identity Changes the chemical composition, resulting in the formation of new substances
No new substance formed New substance formed
Reversible Irreversible

Evidence of Chemical Reactions

  • Heat produced or absorbed
  • Change in pH
  • Gas bubbles form in a liquid
  • Change in color
  • Reactants are used up
  • Precipitate forms in a liquid

Physical and Chemical Properties

Property Type
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

  • Laws describe what happens (observations).
  • Theories explain why something happens.

Atomic Models

  • Thomson's "Plum Pudding" Model: Atoms are a positively charged mass with negatively charged electrons embedded in it.
  • Rutherford's "Planetary" Model: Most of the atom's mass is concentrated in a central nucleus.
  • Bohr's Atomic Model: Electrons orbit the nucleus in fixed pathways (energy levels).
  • Electron Cloud Model: Electrons behave like waves, and their exact location cannot be precisely determined; probability distributions describe regions of likely electron location.

Elements and Atoms

  • An element is a pure substance composed of one type of atom, examples are oxygen, gold, hydrogen.

Components of an Atom

  • Proton: Positive charge, found in the nucleus.
  • Neutron: Neutral charge, found in the nucleus.
  • Electron: Negative charge, orbits the nucleus.

Atomic Number and Mass

  • Atomic number equals the number of protons and electrons in a neutral atom.
  • Atomic mass is the sum of protons and neutrons.

Fluorine Atom

  • Fluorine has 9 protons and 9 electrons.

Fluorine Atom vs. Fluoride Ion

  • Fluoride has gained an electron and carries a -1 charge, fluorine has 9 protons and 7 electrons.

Periodic Table

  • Dmitri Mendeleev developed the periodic table by arranging elements in order of increasing atomic number.

Reactivity of Elements

  • Most reactive: Metals and nonmetals.
  • Least reactive: noble gases.

Properties of Elements

Property Metals Nonmetals Metalloids
State at room temp. Solid (except Hg) Various (solid, liquid, gas) Solid
Appearance Shiny lustre Often dull Can be shiny or dull
Conductivity Good conductors of heat and electricity Poor conductors of heat and electricity May conduct electricity, usually poor conductors of heat
Malleability and ductility Malleable and ductile Brittle, not ductile Brittle, not ductile

Compound Formulas

  • Hâ‚‚O(g): Hydrogen, oxygen. 3 atoms
  • COâ‚‚(g): Carbon, oxygen. 3 atoms
  • Feâ‚‚O₃(s): Iron, oxygen. 5 atoms
  • HCl(l): Hydrogen, chlorine. 2 atoms

Ionic vs. Molecular Compounds

  • Ionic: Metal and nonmetal bonded via ionic bonds.
  • Molecular: Nonmetal and nonmetal bonded via covalent bonds.

Compound Naming

  • Molecular compounds use prefixes (mono, di, tri).
  • Ionic compounds use cation and anion names.

Chemical Equations

  • Reactants: Substances that react.
  • Products: Substances formed from a reaction.

Examples of Chemical Reactions

  • Formation: Two or more reactants combine to form one product.
  • Decomposition: One compound breaks down into two or more simpler substances.
  • Single replacement: One element replaces another element in a compound.
  • Double replacement: The cations and anions of two compounds swap places.
  • Combustion: A substance reacts with oxygen, releasing energy.

Reaction Rates

  • Factors affecting reaction rate: Heat, stirring, reactant concentration, surface area, catalyst.

  • Catalyst: A substance that speeds up a reaction without being consumed.

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