Chapter Menu Lesson 1: Atoms—Basic Units of Matter Lesson 2: Discovering Parts of the Atom Lesson 3: Elements, Isotopes, and Ions—How Atoms Differ Click on a hyperlink to view the corresponding lesson.

4.1 Atoms—Basic Units of Matter nucleus proton neutron electron

What is the current atomic model? 4.1 Atoms—Basic Units of Matter What is the current atomic model? Matter is everything that has mass and takes up space, such as gases, solids, and liquids. Matter is not sound, heat, or light—these are forms of energy. An atom is a very small particle that makes up all matter.

Parts of the Atom Atomic-force microscopes show the surfaces of atoms. 4.1 Atoms—Basic Units of Matter Parts of the Atom Atomic-force microscopes show the surfaces of atoms. The nucleus is the region located in the center of the atom. A particle with a positive charge is a proton. A particle with a negative charge is an electron. A neutron has no charge.

Parts of the Atom (cont.) 4.1 Atoms—Basic Units of Matter Parts of the Atom (cont.)

Parts of the Atom (cont.) 4.1 Atoms—Basic Units of Matter Parts of the Atom (cont.)

4.1 Atoms—Basic Units of Matter The Size of Atoms Protons, neutrons, and electrons are all smaller than the atom.

Historical Evidence of Atoms 4.1 Atoms—Basic Units of Matter Historical Evidence of Atoms Democritus (460–370 B.C.) was the first to propose that atoms were indivisible solid spheres with no holes.

The Law of Conservation of Mass 4.1 Atoms—Basic Units of Matter The Law of Conservation of Mass A chemical reaction rearranges atoms of one substance into another substance with different properties. The total mass of the starting materials is always equal to the total mass of the product.

The Law of Definite Proportions 4.1 Atoms—Basic Units of Matter The Law of Definite Proportions Any pure compound always contains the same elements in the same proportion. Water from your kitchen is the same as water in a glacier on Mars. H2O: two hydrogen atoms and one oxygen atom

Dalton’s Atomic Model 1. All matter is made up of atoms. 4.1 Atoms—Basic Units of Matter Dalton’s Atomic Model 1. All matter is made up of atoms. 2. Atoms are neither created nor destroyed in chemical reactions. 3. Atoms of different elements combine in whole-number ratios. 4. Each element is made of a different kind of atom. 5. The atoms of different elements have different masses and properties.

Dalton’s Atomic Model (cont.) 4.1 Atoms—Basic Units of Matter Dalton’s Atomic Model (cont.)

Which is NOT a particle in an atom? A positron B neutron C electron 4.1 Atoms—Basic Units of Matter A B C D Which is NOT a particle in an atom? A positron B neutron C electron D proton Lesson 1 Review

A Dalton’s atomic model B the law of conservation of mass 4.1 Atoms—Basic Units of Matter A B C D Which law states that the total mass of the starting materials equals the total mass of the product in a chemical reaction? A Dalton’s atomic model B the law of conservation of mass C the law of definite proportions D Democritus’ law Lesson 1 Review

____ make up the nucleus of an atom. A Protons and electrons 4.1 Atoms—Basic Units of Matter A B C D ____ make up the nucleus of an atom. A Protons and electrons B Neutrons and electrons C Protons and neutrons D Neutrons and photons Lesson 1 Review

End of Lesson 1

4.2 Discovering Parts of the Atom spectral lines energy level electron cloud

How were electrons discovered? 4.2 Discovering Parts of the Atom How were electrons discovered? Scientists have put together a detailed model of atoms and their parts. Cathode-ray tubes were used in early experiments on atoms.

How were electrons discovered? (cont.) 4.2 Discovering Parts of the Atom How were electrons discovered? (cont.) A cathode ray is a stream of particles that can be seen when an electric current passes through a vacuum tube. The ray travels from a negatively charged disk at one end to a positively charged disk at the other end.

Thomson’s Experiments 4.2 Discovering Parts of the Atom Thomson’s Experiments Thomson discovered the cathode rays did not travel in a straight line, but bent towards the positively charged plate.

Thomson’s Experiments (cont.) 4.2 Discovering Parts of the Atom Thomson’s Experiments (cont.) Opposite charges attract each other. Thomson concluded the cathode ray must have a negative charge and named the particles electrons.

Thomson’s Atomic Model 4.2 Discovering Parts of the Atom Thomson’s Atomic Model Thomson proposed that an atom was a positively charged sphere. Electrons mixed in to balance the charge.

Discovering the Nucleus 4.2 Discovering Parts of the Atom Discovering the Nucleus In Rutherford’s gold foil experiment, particles were shot through a thin sheet of gold into a detector behind the foil.

Discovering the Nucleus (cont.) 4.2 Discovering Parts of the Atom Discovering the Nucleus (cont.) Rutherford predicted the path of the particles would bend only slightly because the particles would not come upon a charge large enough to strongly repel them.

Discovering the Nucleus (cont.) 4.2 Discovering Parts of the Atom Discovering the Nucleus (cont.) Most of the particles did pass straight though. Some particles were strongly bounced to the side. One in about 8000 bounced completely backwards.

Discovering the Nucleus (cont.) 4.2 Discovering Parts of the Atom Discovering the Nucleus (cont.) If the positive charge was spread evenly, all the particles would have passed through the foil with only a small direction change. Only something with a larger mass and positive charge could cause some of the particles to bounce backwards.

Rutherford’s Atomic Model 4.2 Discovering Parts of the Atom Rutherford’s Atomic Model

Rutherford’s Atomic Model (cont.) 4.2 Discovering Parts of the Atom Rutherford’s Atomic Model (cont.) The positively charged nucleus is in the center of an atom. Electrons with a negative charge travel around empty space surrounding the nucleus.

Completing Rutherford’s Model 4.2 Discovering Parts of the Atom Completing Rutherford’s Model Rutherford also discovered the proton, a particle with a positive charge. Rutherford knew the mass of a proton, but could not account for the total mass of an atom. Rutherford’s theory was later confirmed when the existence of the neutron—a neutral atomic particle with a mass similar to a proton but without a charge—was proved.

Weakness in the Rutherford Model 4.2 Discovering Parts of the Atom Weakness in the Rutherford Model How are electrons arranged? Why do different elements have different chemical properties? Why are some elements more reactive than others?

Bohr and the Hydrogen Atom 4.2 Discovering Parts of the Atom Bohr and the Hydrogen Atom Rutherford thought the electrons moved around the nucleus like a ball swinging on a rope at any distance. Bohr thought electrons traveled in circles with a certain diameter.

Bohr and the Hydrogen Atom (cont.) 4.2 Discovering Parts of the Atom Bohr and the Hydrogen Atom (cont.) Bohr studied hydrogen because it has only one electron. When atoms are excited, they absorb and release energy as light.

The Spectrum of Hydrogen 4.2 Discovering Parts of the Atom The Spectrum of Hydrogen Light passing through a prism is broken into a continuous spectrum of light—red, orange, yellow, green, blue, and violet blend into each other.

The Spectrum of Hydrogen (cont.) 4.2 Discovering Parts of the Atom The Spectrum of Hydrogen (cont.) Ultraviolet rays have shorter wavelengths and higher energies than visible light. Infrared light has longer wavelengths and lower energies than visible light.

The Spectrum of Hydrogen (cont.) 4.2 Discovering Parts of the Atom The Spectrum of Hydrogen (cont.) When excited, hydrogen and neon give off unique narrow bands of light on the spectrum that are called spectral lines.

Spectral Lines and Energy Levels 4.2 Discovering Parts of the Atom Spectral Lines and Energy Levels Each color in a spectral line is a different wavelength and different energy. Electrons can have only certain amounts of energy. Electrons can only move at a certain distance from the nucleus that corresponds to that amount of energy.

Spectral Lines and Energy Levels (cont.) 4.2 Discovering Parts of the Atom Spectral Lines and Energy Levels (cont.) The region in space that an electron can move about the nucleus is called the energy level.

Electrons in the Bohr Atom 4.2 Discovering Parts of the Atom Electrons in the Bohr Atom The electrons can move only in an orbit that is a set distance from the nucleus. Each energy level can hold a certain number of electrons. Bohr’s Model

Electrons in the Bohr Atom (cont.) 4.2 Discovering Parts of the Atom Electrons in the Bohr Atom (cont.) Electrons fill the energy levels in order. The lowest level is filled first. The second level has no electrons until the first level is full. The first level holds 2 electrons, the second level holds 8 electrons. The last energy level may or may not be filled.

Electrons in the Bohr Atom (cont.) 4.2 Discovering Parts of the Atom Electrons in the Bohr Atom (cont.) This diagram shows how electrons are placed in the elements with atomic numbers 1–10.

Bohr’s Model and Chemical Properties 4.2 Discovering Parts of the Atom Bohr’s Model and Chemical Properties Elements have different chemical properties because they have different numbers of electrons in their outer energy level.

Bohr’s Model and Chemical Properties 4.2 Discovering Parts of the Atom Bohr’s Model and Chemical Properties (cont.) Unreactive elements have the exact number of electrons needed to fill their outer energy level. Elements with incomplete outer energy levels are likely to form compounds.

Limitations of Bohr’s Model 4.2 Discovering Parts of the Atom Limitations of Bohr’s Model Energy levels were like circular orbits. Bohr’s theory works for the simple hydrogen atom, but not for more complex elements. Atomic Model

The Electron Cloud Model 4.2 Discovering Parts of the Atom The Electron Cloud Model The electron cloud is the region surrounding an atomic nucleus where an electron is most likely to be found. Electrons are more likely to be near the nucleus because they are attracted to the positive charge of the protons. Electron Cloud Model

An excited hydrogen atom emits narrow bands of light called ____. 4.2 Discovering Parts of the Atom A B C D An excited hydrogen atom emits narrow bands of light called ____. A energy lines B wave lines C spectral lines D wavelengths Lesson 2 Review

Elements that do not react with other elements must have ____. 4.2 Discovering Parts of the Atom A B C D Elements that do not react with other elements must have ____. A completely filled energy levels B excited electrons C empty energy levels D the same number of protons and neutrons Lesson 2 Review

A because they were repelled by the protons in the foil 4.2 Discovering Parts of the Atom A B C D In the gold foil experiment, why did some particles pass straight through the foil? A because they were repelled by the protons in the foil B because they were attracted by the protons in the foil C because atoms have no effect on charged particles D because atoms are mostly empty spaces Lesson 2 Review

End of Lesson 2

4.3 Elements, Isotopes, and Ions—How Atoms Differ atomic number mass number isotope average atomic mass ion

Different Elements— Different Numbers of Protons 4.3 Elements, Isotopes, and Ions—How Atoms Differ Different Elements— Different Numbers of Protons An element is a pure substance made from atoms that all have the same number of protons. Atoms of a particular element always have the same number of protons.

Different Elements— Different Numbers of Protons (cont.) 4.3 Elements, Isotopes, and Ions—How Atoms Differ Different Elements— Different Numbers of Protons (cont.) The number of protons in an atom of an element is the element’s atomic number. How can you tell which elements form chemical bonds?

Atomic Number and the Periodic Table 4.3 Elements, Isotopes, and Ions—How Atoms Differ Atomic Number and the Periodic Table The periodic table shows elements that increase in atomic number horizontally. Elements in the same column have similar properties. Most of the elements on the periodic table are metals.

Atomic Number and the Periodic Table (cont.)

Atomic Number and the Periodic Table (cont.) 4.3 Elements, Isotopes, and Ions—How Atoms Differ Atomic Number and the Periodic Table (cont.)

Isotopes—Different Numbers of Neutrons 4.3 Elements, Isotopes, and Ions—How Atoms Differ Isotopes—Different Numbers of Neutrons Atoms of the same element always have the same number of protons, but they may have different numbers of neutrons. Isotopes

Protons, Neutrons, and Mass Number 4.3 Elements, Isotopes, and Ions—How Atoms Differ Protons, Neutrons, and Mass Number An atom’s mass number is the sum of the number of protons and the number of neutrons. To calculate the number of neutrons, subtract the atomic number from the mass number.

4.3 Elements, Isotopes, and Ions—How Atoms Differ Atoms of the same element that have different numbers of neutrons are called isotopes.

4.3 Elements, Isotopes, and Ions—How Atoms Differ Isotopes (cont.) The average atomic mass of an element is the weighted average mass of the mixture of an element’s isotopes.

4.3 Elements, Isotopes, and Ions—How Atoms Differ Isotopes (cont.) Radioactive isotopes are unstable and break down releasing particles, radiation, and energy.

Isotopes of Hydrogen Hydrogen has three isotopes. 4.3 Elements, Isotopes, and Ions—How Atoms Differ Isotopes of Hydrogen Hydrogen has three isotopes.

Isotopes of Hydrogen (cont.) 4.3 Elements, Isotopes, and Ions—How Atoms Differ Isotopes of Hydrogen (cont.)

Ions—Gaining or Losing Electrons 4.3 Elements, Isotopes, and Ions—How Atoms Differ Ions—Gaining or Losing Electrons Atoms can gain or lose electrons. When an electron is gained or lost, the atom no longer has the same number of electrons as protons. The atom no longer has a neutral charge. An atom that has gained or lost an electron and is no longer neutral is called an ion.

Ions—Gaining or Losing Electrons (cont.)

Positive Ions— Losing Electrons 4.3 Elements, Isotopes, and Ions—How Atoms Differ Positive Ions— Losing Electrons When an atom loses an electron, it has more protons than electrons. The atom has a positive charge and is called a positive ion.

Negative Ions— Gaining Electrons 4.3 Elements, Isotopes, and Ions—How Atoms Differ Negative Ions— Gaining Electrons When an atom gains an electron, it has more electrons than protons. The atom has a negative charge and is called a negative ion. Positive ions and negative ions attract each other and form compounds.

A Carbon-14 has a positive charge. B Carbon-13 has a positive charge. 4.3 Elements, Isotopes, and Ions—How Atoms Differ A B C D The carbon element has several isotopes. How is carbon-14 different from carbon-13? A Carbon-14 has a positive charge. B Carbon-13 has a positive charge. C Carbon-14 has one more neutron than carbon-13. D Carbon-14 has one less neutron than carbon-13. Lesson 3 Review

What is the number of protons in an element called? A isotope 4.3 Elements, Isotopes, and Ions—How Atoms Differ A B C D What is the number of protons in an element called? A isotope B atomic number C atomic mass D radiotope Lesson 3 Review

How does a neutral atom become a negative ion of the same element? 4.3 Elements, Isotopes, and Ions—How Atoms Differ A B C D How does a neutral atom become a negative ion of the same element? A It gains a proton. B It loses a proton. C It loses an electron. D It gains an electron. Lesson 3 Review

End of Lesson 3

Chapter Resources Menu Chapter Assessment California Standards Practice Concepts in Motion Image Bank Science Online Interactive Table Virtual Lab BrainPOP Click on a hyperlink to view the corresponding feature.

Atoms of the same element always have the same number of ____. C D Atoms of the same element always have the same number of ____. A electrons B neutrons C ions D protons Chapter Assessment 1

An electron moves into a higher energy level. What must have happened? B C D An electron moves into a higher energy level. What must have happened? A The electron released energy. B The electron absorbed energy. C The atom gained a negative charge. D The atom gained a positive charge. Chapter Assessment 2

A B C D An atom contains 10 electrons, 11 protons, and 11 neutrons. What is the charge on the atom? A 1− B 1+ C 2− D 2+ Chapter Assessment 3

A B C D Elements with the same number of protons but differing numbers of neutrons are called ____. A ions B electrons C tritium D isotopes Chapter Assessment 4

A spectral line is caused by ____. A an excited electron releasing energy and falling to a lower energy level B an excited electron absorbing electricity and jumping to a higher energy level C an atom gaining an ionic charge D an atom losing a proton Chapter Assessment 5

The atomic mass of an atom is equal to ____. A the number of protons SCI 3.a A B C D The atomic mass of an atom is equal to ____. A the number of protons B the number of neutrons C the number of protons and neutrons D the number of electrons and protons CA Standards Practice 1

The atomic number of carbon is 6. Carbon-14 contains ____. SCI 7.b A B C D The atomic number of carbon is 6. Carbon-14 contains ____. A 7 protons and 7 neutrons B 6 protons and 8 neutrons C 8 protons and 6 neutrons D 6 protons and 6 neutrons CA Standards Practice 2

What happens when an atom gains a negative charge? SCI 3.a A B C D What happens when an atom gains a negative charge? A The atom gains an electron. B The atom gains a proton. C The atom loses an electron. D The atom loses a proton. CA Standards Practice 3

Which particle has a positive charge? A nucleus B proton C electron SCI 3.a A B C D Which particle has a positive charge? A nucleus B proton C electron D neutron CA Standards Practice 4

Who thought that atoms were very small, solid spheres? A Dalton SCI 3.a A B C D Who thought that atoms were very small, solid spheres? A Dalton B Rutherford C Thompson D Democritus CA Standards Practice 5

Concepts in Motion 1

Concepts in Motion 2

Concepts in Motion 3

Image Bank

Image Bank

Interactive Table

End of Resources