The Nature of Matter Section 5-1.

The Nature of Matter Section 5-1

Note-Taking Guide: The Nature of Matter
I. Atom: _____________________________________ A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton 1 neutron negative Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton 1 neutron negative Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 neutron negative Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 neutron no charge negative Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 neutron no charge electron negative Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 neutron no charge electron negative ~0 Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 nucleus neutron no charge electron negative ~0 Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 nucleus neutron no charge electron negative ~0 Outside nucleus Most atoms are neutral because they have equal numbers of ______and _______. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 nucleus neutron no charge electron negative ~0 Outside nucleus Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 nucleus neutron no charge electron negative ~0 Outside nucleus Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a positive charge. Atoms that gain electrons have a ________________ charge.

I. Atom: smallest unit of matter A. Subatomic Particles Particle Charge Relative Mass Location in Atom proton positive 1 nucleus neutron no charge electron negative ~0 Outside nucleus Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a positive charge. Atoms that gain electrons have a negative charge.

I. Element: ______________________________________ A. atomic number: _____________________________ B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________

I. Element: substance made of one type of atom A. atomic number: _____________________________ B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________

I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________

I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________

I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________

I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation) 1. uses: _________________________________ ___________________________________________

I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation) 1. uses: dating fossils, diagnosing and treating diseases, killing bacteria in food/ on surgical equipment

Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 8 neutrons 7 neutrons

III. Compound: _________________________________ ______________________________________________ IV. Chemical Bonds valence electrons: _________________________ ion: ______________________________ B. ionic bond: ___________________________________ ____________________ C. covalent bond: _______________________________ ___________ molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: _________________________ ion: ______________________________ B. ionic bond: ___________________________________ ____________________ C. covalent bond: _______________________________ ___________ molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: outermost electrons in an atom ion: ______________________________ B. ionic bond: ___________________________________ ____________________ C. covalent bond: _______________________________ ___________ molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons B. ionic bond: ___________________________________ ____________________ C. covalent bond: _______________________________ ___________ molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons B. ionic bond: bond formed by the transfer of electrons from one atom to another C. covalent bond: _______________________________ ___________ molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons B. ionic bond: bond formed by the transfer of electrons from one atom to another C. covalent bond: bond formed when atoms share electrons molecule: ___________________________________

III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions IV. Chemical Bonds valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons B. ionic bond: bond formed by the transfer of electrons from one atom to another C. covalent bond: bond formed when atoms share electrons molecule: group of atoms covalently bonded together

Sodium atom (Na) Chlorine atom (Cl) Transfer of electron Protons +11 Electrons -11 Charge Protons +17 Electrons -17

Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-) Transfer of electron Protons +11 Electrons -11 Charge Protons +17 Electrons -17 Electrons -10 Charge Electrons -18 Charge

Periodic Table, Electrons, and Bonding
I. Periodic Table Design: 1. 2. 3. 4. Elements are arranged in order of increasing An element’s position on the periodic table tells you:

I. Periodic Table Design: Each square contains info. about 1 element. 1. 2. 3. 4. Elements are arranged in order of increasing An element’s position on the periodic table tells you:

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. 3. 4. Elements are arranged in order of increasing An element’s position on the periodic table tells you: 1.

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. 4. Elements are arranged in order of increasing An element’s position on the periodic table tells you: 1. 2.

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. element name 4. Elements are arranged in order of increasing An element’s position on the periodic table tells you: 1. 2.

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. element name 4. atomic mass (weighted avg. of the mass # of each isotope) Elements are arranged in order of increasing An element’s position on the periodic table tells you: 1. 2.

6 C Carbon 12.011

6 C Carbon 12.011 Atomic number

6 C Carbon 12.011 Atomic number Element Symbol

6 C Carbon 12.011 Atomic number Element Symbol Element Name

6 C Carbon 12.011 Atomic number Element Symbol Element Name Atomic mass

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. element name 4. atomic mass (weighted avg. of the mass # of each isotope) Elements are arranged in order of increasing atomic number. An element’s position on the periodic table tells you: 1. 2.

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. element name 4. atomic mass (weighted avg. of the mass # of each isotope) Elements are arranged in order of increasing atomic number. An element’s position on the periodic table tells you: 1. chemical and physical properties of the element 2.

I. Periodic Table Design: Each square contains info. about 1 element. 1. atomic number 2. element symbol 3. element name 4. atomic mass (weighted avg. of the mass # of each isotope) Elements are arranged in order of increasing atomic number. An element’s position on the periodic table tells you: 1. chemical and physical properties of the element 2. how the element will bond with other elements

Families: Periods:

Families: vertical columns; elements in the same family have similar properties B. Periods:

Families: vertical columns; elements in the same family have similar properties B. Periods: horizontal rows; elements in the same period do NOT have similar properties

II. Electrons and Orbitals A. orbital: B. Bohr diagram: 1st orbital can hold _ electrons. 2nd orbital can hold _ electrons. 3rd orbital can hold _ electrons.

II. Electrons and Orbitals A. orbital: region in space (outside the nucleus) where electrons are found B. Bohr diagram: 1st orbital can hold _ electrons. 2nd orbital can hold _ electrons. 3rd orbital can hold _ electrons.

II. Electrons and Orbitals A. orbital: region in space (outside the nucleus) where electrons are found B. Bohr diagram: shows which orbitals electrons are found in 1st orbital can hold _ electrons. 2nd orbital can hold _ electrons. 3rd orbital can hold _ electrons.

II. Electrons and Orbitals A. orbital: region in space (outside the nucleus) where electrons are found B. Bohr diagram: shows which orbitals electrons are found in 1st orbital can hold 2 electrons. 2nd orbital can hold _ electrons. 3rd orbital can hold _ electrons.

II. Electrons and Orbitals A. orbital: region in space (outside the nucleus) where electrons are found B. Bohr diagram: shows which orbitals electrons are found in 1st orbital can hold 2 electrons. 2nd orbital can hold 8 electrons. 3rd orbital can hold _ electrons.

II. Electrons and Orbitals A. orbital: region in space (outside the nucleus) where electrons are found B. Bohr diagram: shows which orbitals electrons are found in 1st orbital can hold 2 electrons. 2nd orbital can hold 8 electrons. 3rd orbital can hold 8 electrons.

C. valence electrons: 1. determine 2. elements in the same family have

C. valence electrons: electrons in the outermost orbital of an atom 1. determine 2. elements in the same family have

C. valence electrons: electrons in the outermost orbital of an atom 1. determine the number of bonds and types of bonds that an atom can make 2. elements in the same family have

C. valence electrons: electrons in the outermost orbital of an atom 1. determine the number of bonds and types of bonds that an atom can make 2. elements in the same family have the same number of valence electrons

He: __ F: __ Mg: __ Al: __ 3. Goal: Why? How?

He: 2 F: __ Mg: __ Al: __ 3. Goal: Why? How?

He: 2 F: 7 Mg: __ Al: __ 3. Goal: Why? How?

He: 2 F: 7 Mg: 2 Al: __ 3. Goal: Why? How?

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: Why? How?

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? How?

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? Stable state (unreactive) – like noble gases in last family on the periodic table How?

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? Stable state (unreactive) – like noble gases in last family on the periodic table How? Gain or lose electrons

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? Stable state (unreactive) – like noble gases in last family on the periodic table How? Gain or lose electrons Atoms that gain electrons form ________ ions. Atoms that lose electrons form ________ ions.

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? Stable state (unreactive) – like noble gases in last family on the periodic table How? Gain or lose electrons Atoms that gain electrons form negative ions. Atoms that lose electrons form ________ ions.

He: 2 F: 7 Mg: 2 Al: 3 3. Goal: a full outermost orbital Why? Stable state (unreactive) – like noble gases in last family on the periodic table How? Gain or lose electrons Atoms that gain electrons form negative ions. Atoms that lose electrons form positive ions.

4. Generalizations a. Atoms on the left side of the periodic table tend to ____ electrons to form ________ ions. b. Atoms on the right side of the periodic table tend to ____ electrons to form ________ ions.

4. Generalizations a. Atoms on the left side of the periodic table tend to lose electrons to form ________ ions. b. Atoms on the right side of the periodic table tend to ____ electrons to form ________ ions.

4. Generalizations a. Atoms on the left side of the periodic table tend to lose electrons to form positive ions. b. Atoms on the right side of the periodic table tend to ____ electrons to form ________ ions.

4. Generalizations a. Atoms on the left side of the periodic table tend to lose electrons to form positive ions. b. Atoms on the right side of the periodic table tend to gain electrons to form ________ ions.

4. Generalizations a. Atoms on the left side of the periodic table tend to lose electrons to form positive ions. b. Atoms on the right side of the periodic table tend to gain electrons to form negative ions.

You can use the periodic table to determine the charge on the ion.

III. Bonding:

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons.

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to ______ electron Chlorine wants to ______ electron 2. Hydrogen wants to ______ electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to ______ electron 2. Hydrogen wants to ______ electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron 2. Hydrogen wants to ______ electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  2. Hydrogen wants to ______ electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to ______ electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to lose 1 electron Oxygen wants to ______ electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to lose 1 electron Oxygen wants to gain 2 electrons

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to lose 1 electron Oxygen wants to gain 2 electrons H + O 

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to lose 1 electron Oxygen wants to gain 2 electrons H + O  H2O

III. Bonding: Atoms that want to gain electrons tend to form bonds with atoms that want to lose electrons. Examples: Sodium wants to lose 1 electron Chlorine wants to gain 1 electron Na + Cl  NaCl 2. Hydrogen wants to lose 1 electron Oxygen wants to gain 2 electrons 2H2 + O2  2H2O

The Nature of Matter Section 5-1.

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