A brief power point presentation designed to help introduce high school chemistry students to reading the periodic table and extracting information such as the number of valence electrons an element has, etc.
This document summarizes various chemistry concepts related to bonding:
1) Atoms bond through ionic bonding, where ions with opposite charges attract, or covalent bonding, where electrons are shared between atoms.
2) Ionic bonds form between ions, while covalent bonds form when atoms share electrons to achieve stable full outer energy levels.
3) Bonding diagrams like Lewis structures are used to represent how atoms bond by sharing or transferring electrons to achieve stable configurations.
The document discusses the periodic table and properties of elements. It explains that each row of the periodic table is called a period, with elements in the same period having the same number of electron shells. It also explains that each column is called a group, with elements in the same group having the same number of valence electrons in their outer shell. The document provides examples of determining the number of shells and valence electrons for various elements based on their period and group.
1. Hydrogen has one valence electron and is not an alkali metal.
2. The alkali metals have one valence electron.
3. The transition metals are harder than the alkali metals.
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
This document discusses the molecular structure of atoms. It begins by explaining that all substances are composed of elements, which are the basic substances, and that elements are made up of very small particles called atoms. It then describes the basic structure of an atom, including that atoms have a small, positively charged nucleus surrounded by negatively charged electrons. The number of protons determines the element and equals the number of electrons. Atoms can gain, lose, or share electrons to attain stable electron configurations, forming ions or molecules.
This document is a worksheet about valence electrons that contains questions asking students to:
1) Identify the number of electrons in various elements.
2) Draw Lewis structures and identify the number of outer shell electrons for different elements.
3) Identify the number of valence electrons elements have by filling in their electron configurations.
Each row of the periodic table is called a period. Elements in the same period have the same number of electron shells. Each column is called a group. Elements in the same group have the same number of valence electrons, except for helium which has two electrons. Valence electrons are the outermost electrons of an atom and are involved in bonding. Reactive elements bond easily to gain or lose valence electrons to achieve a full outer electron shell of eight electrons.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
This document summarizes various chemistry concepts related to bonding:
1) Atoms bond through ionic bonding, where ions with opposite charges attract, or covalent bonding, where electrons are shared between atoms.
2) Ionic bonds form between ions, while covalent bonds form when atoms share electrons to achieve stable full outer energy levels.
3) Bonding diagrams like Lewis structures are used to represent how atoms bond by sharing or transferring electrons to achieve stable configurations.
The document discusses the periodic table and properties of elements. It explains that each row of the periodic table is called a period, with elements in the same period having the same number of electron shells. It also explains that each column is called a group, with elements in the same group having the same number of valence electrons in their outer shell. The document provides examples of determining the number of shells and valence electrons for various elements based on their period and group.
1. Hydrogen has one valence electron and is not an alkali metal.
2. The alkali metals have one valence electron.
3. The transition metals are harder than the alkali metals.
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
This document discusses the molecular structure of atoms. It begins by explaining that all substances are composed of elements, which are the basic substances, and that elements are made up of very small particles called atoms. It then describes the basic structure of an atom, including that atoms have a small, positively charged nucleus surrounded by negatively charged electrons. The number of protons determines the element and equals the number of electrons. Atoms can gain, lose, or share electrons to attain stable electron configurations, forming ions or molecules.
This document is a worksheet about valence electrons that contains questions asking students to:
1) Identify the number of electrons in various elements.
2) Draw Lewis structures and identify the number of outer shell electrons for different elements.
3) Identify the number of valence electrons elements have by filling in their electron configurations.
Each row of the periodic table is called a period. Elements in the same period have the same number of electron shells. Each column is called a group. Elements in the same group have the same number of valence electrons, except for helium which has two electrons. Valence electrons are the outermost electrons of an atom and are involved in bonding. Reactive elements bond easily to gain or lose valence electrons to achieve a full outer electron shell of eight electrons.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
This chapter discusses ionic bonding. It begins by explaining that noble gases have a stable electronic configuration with a full outer shell. Most other elements form ions by gaining or losing electrons to achieve a noble gas configuration. Ionic bonds form when metals transfer electrons to non-metals to form positively charged cations and negatively charged anions. Ionic compounds have a crystalline structure where the ions are arranged in a repeating pattern with strong electrostatic forces between them. This results in ionic compounds having high melting points, being insoluble in organic solvents, and capable of conducting electricity when molten or dissolved in water.
This document provides an overview of chemical bonding concepts including:
- The octet rule which states that main group elements form ions to achieve 8 valence electrons.
- Ionic and covalent bonds are formed through the transfer or sharing of electrons respectively.
- Lewis structures are used to represent electron pairing in molecules and predict molecular geometry based on electron pair repulsion.
This document discusses ionic bonding between atoms. It explains that ionic bonds form when a metal atom donates one or more electrons to a nonmetal atom, giving the metal a positive charge and the nonmetal a negative charge. The document outlines how main group elements gain or lose electrons to achieve a full outer shell of 8 electrons, and provides the example of sodium donating an electron to chlorine to form ionic bonded sodium and chloride ions.
1. The document discusses the chemical bonding concepts of Lewis dot structures, valence electrons, electronegativity, and ionization energy. It describes an activity where students draw Lewis dot structures of elements and organize them based on these properties.
2. Gilbert Lewis is credited with discovering covalent bonds and representing atoms with Lewis dot structures that show valence electrons. His work established that chemical bonds form through the transfer or sharing of electrons between atoms.
3. The document guides students to draw Lewis dot structures, identify trends in valence electrons, electronegativity, and ionization energy for different elements, and recognize how these properties relate to bond formation.
This document discusses how to determine if an atom is a metal or non-metal based on its valence electrons, and describes the formation of ionic and covalent bonds. Ionic bonds form between metal and non-metal atoms through the transfer of electrons from the metal to the non-metal. Covalent bonds form between non-metal atoms through the sharing of electrons. Examples of ionic bond formation in sodium chloride and covalent bond formation in carbon dioxide are provided, along with electron diagrams to illustrate bonding.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
This document discusses valence electrons and how to determine the number available for bonding using the periodic table. It defines valence electrons as those in the outermost shell or energy level available for bonding. It provides examples of how many valence electrons elements in different groups have, from 1 to 8. It also introduces Lewis dot structures as a way to represent an atom's valence electrons and provides examples of Lewis dot structures for period 2 elements.
This document provides an overview of physical science concepts related to subatomic particles, the periodic table, oxidation numbers, and Lewis dot diagrams. The key points are:
1) It reviews subatomic particles, periods and groups of the periodic table, and electron configurations.
2) The objective is to predict oxidation numbers and draw Lewis dot diagrams by understanding valence electrons.
3) It defines valence electrons, oxidation numbers, and ionic bonds in chemical compounds.
4) Examples are given of writing chemical symbols, determining valence electrons, and drawing Lewis dot diagrams using the cross method.
Limestone is a naturally occurring resource that is quarried and used to make cement, concrete, and other building materials. It is composed mainly of calcium carbonate, which can be decomposed through heating to calcium oxide and carbon dioxide. Calcium oxide reacts with water to form calcium hydroxide, which is used to neutralize acidic soils. Metals are extracted from metal ores through various processes like heating with carbon or electrolysis depending on the reactivity of the metal. New extraction methods are being developed as metal ores become depleted.
Sue welcomes viewers to her new show. The show stars Sue and will feature her talents and skills. Sue is excited to entertain audiences and show off her abilities on television. Viewers are sure to enjoy Sue's unique personality and performance.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
Ionic bonds form when electrons are transferred from a metal atom to a non-metal atom, creating oppositely charged ions. Covalent bonds form through the sharing of electrons between non-metal atoms. Ionic compounds contain ionic bonds and transfer electrons, while covalent compounds share electrons. Examples of ionic compounds are sodium chloride and magnesium oxide, while examples of covalent compounds are hydrogen gas, oxygen gas, and carbon dioxide. Ionic compounds are generally solids with high melting points that conduct electricity when molten or dissolved, while covalent compounds can be solids, liquids or gases with varied properties depending on molecular complexity.
1) The document discusses Lewis structures, which are diagrams that show how valence electrons are shared between atoms to form chemical bonds.
2) It explains valence bond theory and the octet rule, which states that atoms are most stable when their valence shell contains 8 electrons.
3) The document provides steps for drawing Lewis structures for different types of compounds, including elements, binary covalent compounds, compounds with multiple bonds, and polyatomic ions.
Visiting a volcano would be the better class field trip for three reasons:
1) Volcanoes demonstrate geological processes like lava flows and eruptions that help students learn earth science.
2) Seeing volcanic landscapes up close helps students understand how volcanoes shape the environment.
3) Volcanoes present hazards but are also sites of new land being formed, offering learning opportunities about geological cycles.
The document discusses ionic compounds and their properties. It defines ionic compounds as formed from positively and negatively charged ions. Sodium chloride is given as an example where sodium loses an electron to become Na+ and chlorine gains an electron to become Cl-. Ionic compounds form crystalline structures and dissolve into ions in water, allowing them to conduct electricity. Common polyatomic ions are also discussed.
The document provides information about the structure of atoms and the periodic table. It discusses the subatomic particles that make up atoms, including electrons, protons, and neutrons. It then explains atomic structure and how elements are arranged on the periodic table according to their atomic number and properties. Various types of bonding between atoms are introduced, including ionic and covalent bonding. Bonding diagrams and examples of different compounds are provided.
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
Lesson 8Chemical Bonding & NomenclatureYou should view all.docxsmile790243
Lesson 8
Chemical Bonding & Nomenclature
You should view all lectures as a slide show. In the toolbar above, click “Slide Show” and “From Beginning” to start. Hit the space bar to forward to next slide or item.
1
*Read: Watch the Lecture as a slideshow, hit the space bar to move forward or just left click.
1
Topics:
Chemical Bonds
Lewis Dot Structures
Molecular Geometry
Polar Bonds
Naming Compounds
Writing Chemical Formulas
Naming Molecular Compounds
Lesson 8: Chemical Bonding and Nomenclature
2
2
Chemical Bonds
Sodium (Na) is a silver-colored metal that reacts so
violently with water that flames are produced when sodium
gets wet.
Chlorine (Cl) is a greenish-colored gas that is so poisonous that it was used as a weapon in World War I.
When the electrons of sodium metal and chlorine gas interact, the compound sodium chloride (NaCl) is formed, which is table salt.
Since the body is over 90% water, ingesting sodium metal would literally set someone on fire!
If we make a compound out of Na, we can make something totally different such as the table salt used to season our food.
3
Chemical Bonds
Atoms can interact with each other to form new substances called
compounds.
Compounds are formed when electrons in an atom’s last energy level interact and form chemical bonds. A chemical bond is an attractive force between atoms that holds them together.
An atom’s outermost energy level of electrons is called the valence shell (or valence level) and the electrons in the valence shell are called valence electrons.
4
Na Atom
Cl Atom
Sodium has 1 valence electron in the valence shell.
Chlorine has 7 valence electron in the valence shell.
Chemical Bonds
In ionic bonds, metals always lose electrons to nonmetals and become positive (or cations).
In ionic bonds, nonmetals always attract electrons from metals and become negative (anions).
Ionic compounds are neutral compounds made up of cations and anions.
Covalent bonds are formed between nonmetals and electrons are shared so no ions are formed.
Cl
nonmetal
Na
metal
O
nonmetal
O
nonmetal
Metal + Nonmetal = Ionic Compound
Nonmetal + Nonmetal = Covalent Compound
Chemical Bonds: Ionic
The octet rule states that atoms will gain, lose, or share
valence electrons in a way that will give each atom eight electrons in their valence shell.
Na has 1 electron in its valence shell and Cl has 7 electrons in its valence shell. Cl needs 1 valence electron to have 8 in its outer shell.
If Na transfers its 1 valence electron to Cl, Na’s second energy level becomes the valence shell, which already has 8 electrons.
Now, Na has a positive 1 charge and Cl has a negative 1 charge. But, the charge on NaCl is zero (the charges cancel each other out).
6
Na Atom
Cl Atom
Ionic Bond
Chemical Bonds: Ionic
An Ionic bond is formed when there is a transfer of electrons from a metal to a nonmetal. Compounds formed by ionic bonds are ...
The document discusses atomic structure and ions. It defines isotopes as atoms of the same element with different numbers of neutrons. The outermost electrons of an atom are involved in chemical reactions. The periodic table arranges elements by their number of outermost electrons. Noble gases have full outermost shells with 2 or 8 electrons. Atoms form ions by gaining or losing electrons to achieve stable configurations. Positively charged ions are formed when electrons are lost, and negatively charged ions are formed when electrons are gained.
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
This chapter discusses ionic bonding. It begins by explaining that noble gases have a stable electronic configuration with a full outer shell. Most other elements form ions by gaining or losing electrons to achieve a noble gas configuration. Ionic bonds form when metals transfer electrons to non-metals to form positively charged cations and negatively charged anions. Ionic compounds have a crystalline structure where the ions are arranged in a repeating pattern with strong electrostatic forces between them. This results in ionic compounds having high melting points, being insoluble in organic solvents, and capable of conducting electricity when molten or dissolved in water.
This document provides an overview of chemical bonding concepts including:
- The octet rule which states that main group elements form ions to achieve 8 valence electrons.
- Ionic and covalent bonds are formed through the transfer or sharing of electrons respectively.
- Lewis structures are used to represent electron pairing in molecules and predict molecular geometry based on electron pair repulsion.
This document discusses ionic bonding between atoms. It explains that ionic bonds form when a metal atom donates one or more electrons to a nonmetal atom, giving the metal a positive charge and the nonmetal a negative charge. The document outlines how main group elements gain or lose electrons to achieve a full outer shell of 8 electrons, and provides the example of sodium donating an electron to chlorine to form ionic bonded sodium and chloride ions.
1. The document discusses the chemical bonding concepts of Lewis dot structures, valence electrons, electronegativity, and ionization energy. It describes an activity where students draw Lewis dot structures of elements and organize them based on these properties.
2. Gilbert Lewis is credited with discovering covalent bonds and representing atoms with Lewis dot structures that show valence electrons. His work established that chemical bonds form through the transfer or sharing of electrons between atoms.
3. The document guides students to draw Lewis dot structures, identify trends in valence electrons, electronegativity, and ionization energy for different elements, and recognize how these properties relate to bond formation.
This document discusses how to determine if an atom is a metal or non-metal based on its valence electrons, and describes the formation of ionic and covalent bonds. Ionic bonds form between metal and non-metal atoms through the transfer of electrons from the metal to the non-metal. Covalent bonds form between non-metal atoms through the sharing of electrons. Examples of ionic bond formation in sodium chloride and covalent bond formation in carbon dioxide are provided, along with electron diagrams to illustrate bonding.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
This document discusses valence electrons and how to determine the number available for bonding using the periodic table. It defines valence electrons as those in the outermost shell or energy level available for bonding. It provides examples of how many valence electrons elements in different groups have, from 1 to 8. It also introduces Lewis dot structures as a way to represent an atom's valence electrons and provides examples of Lewis dot structures for period 2 elements.
This document provides an overview of physical science concepts related to subatomic particles, the periodic table, oxidation numbers, and Lewis dot diagrams. The key points are:
1) It reviews subatomic particles, periods and groups of the periodic table, and electron configurations.
2) The objective is to predict oxidation numbers and draw Lewis dot diagrams by understanding valence electrons.
3) It defines valence electrons, oxidation numbers, and ionic bonds in chemical compounds.
4) Examples are given of writing chemical symbols, determining valence electrons, and drawing Lewis dot diagrams using the cross method.
Limestone is a naturally occurring resource that is quarried and used to make cement, concrete, and other building materials. It is composed mainly of calcium carbonate, which can be decomposed through heating to calcium oxide and carbon dioxide. Calcium oxide reacts with water to form calcium hydroxide, which is used to neutralize acidic soils. Metals are extracted from metal ores through various processes like heating with carbon or electrolysis depending on the reactivity of the metal. New extraction methods are being developed as metal ores become depleted.
Sue welcomes viewers to her new show. The show stars Sue and will feature her talents and skills. Sue is excited to entertain audiences and show off her abilities on television. Viewers are sure to enjoy Sue's unique personality and performance.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
Ionic bonds form when electrons are transferred from a metal atom to a non-metal atom, creating oppositely charged ions. Covalent bonds form through the sharing of electrons between non-metal atoms. Ionic compounds contain ionic bonds and transfer electrons, while covalent compounds share electrons. Examples of ionic compounds are sodium chloride and magnesium oxide, while examples of covalent compounds are hydrogen gas, oxygen gas, and carbon dioxide. Ionic compounds are generally solids with high melting points that conduct electricity when molten or dissolved, while covalent compounds can be solids, liquids or gases with varied properties depending on molecular complexity.
1) The document discusses Lewis structures, which are diagrams that show how valence electrons are shared between atoms to form chemical bonds.
2) It explains valence bond theory and the octet rule, which states that atoms are most stable when their valence shell contains 8 electrons.
3) The document provides steps for drawing Lewis structures for different types of compounds, including elements, binary covalent compounds, compounds with multiple bonds, and polyatomic ions.
Visiting a volcano would be the better class field trip for three reasons:
1) Volcanoes demonstrate geological processes like lava flows and eruptions that help students learn earth science.
2) Seeing volcanic landscapes up close helps students understand how volcanoes shape the environment.
3) Volcanoes present hazards but are also sites of new land being formed, offering learning opportunities about geological cycles.
The document discusses ionic compounds and their properties. It defines ionic compounds as formed from positively and negatively charged ions. Sodium chloride is given as an example where sodium loses an electron to become Na+ and chlorine gains an electron to become Cl-. Ionic compounds form crystalline structures and dissolve into ions in water, allowing them to conduct electricity. Common polyatomic ions are also discussed.
The document provides information about the structure of atoms and the periodic table. It discusses the subatomic particles that make up atoms, including electrons, protons, and neutrons. It then explains atomic structure and how elements are arranged on the periodic table according to their atomic number and properties. Various types of bonding between atoms are introduced, including ionic and covalent bonding. Bonding diagrams and examples of different compounds are provided.
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
Lesson 8Chemical Bonding & NomenclatureYou should view all.docxsmile790243
Lesson 8
Chemical Bonding & Nomenclature
You should view all lectures as a slide show. In the toolbar above, click “Slide Show” and “From Beginning” to start. Hit the space bar to forward to next slide or item.
1
*Read: Watch the Lecture as a slideshow, hit the space bar to move forward or just left click.
1
Topics:
Chemical Bonds
Lewis Dot Structures
Molecular Geometry
Polar Bonds
Naming Compounds
Writing Chemical Formulas
Naming Molecular Compounds
Lesson 8: Chemical Bonding and Nomenclature
2
2
Chemical Bonds
Sodium (Na) is a silver-colored metal that reacts so
violently with water that flames are produced when sodium
gets wet.
Chlorine (Cl) is a greenish-colored gas that is so poisonous that it was used as a weapon in World War I.
When the electrons of sodium metal and chlorine gas interact, the compound sodium chloride (NaCl) is formed, which is table salt.
Since the body is over 90% water, ingesting sodium metal would literally set someone on fire!
If we make a compound out of Na, we can make something totally different such as the table salt used to season our food.
3
Chemical Bonds
Atoms can interact with each other to form new substances called
compounds.
Compounds are formed when electrons in an atom’s last energy level interact and form chemical bonds. A chemical bond is an attractive force between atoms that holds them together.
An atom’s outermost energy level of electrons is called the valence shell (or valence level) and the electrons in the valence shell are called valence electrons.
4
Na Atom
Cl Atom
Sodium has 1 valence electron in the valence shell.
Chlorine has 7 valence electron in the valence shell.
Chemical Bonds
In ionic bonds, metals always lose electrons to nonmetals and become positive (or cations).
In ionic bonds, nonmetals always attract electrons from metals and become negative (anions).
Ionic compounds are neutral compounds made up of cations and anions.
Covalent bonds are formed between nonmetals and electrons are shared so no ions are formed.
Cl
nonmetal
Na
metal
O
nonmetal
O
nonmetal
Metal + Nonmetal = Ionic Compound
Nonmetal + Nonmetal = Covalent Compound
Chemical Bonds: Ionic
The octet rule states that atoms will gain, lose, or share
valence electrons in a way that will give each atom eight electrons in their valence shell.
Na has 1 electron in its valence shell and Cl has 7 electrons in its valence shell. Cl needs 1 valence electron to have 8 in its outer shell.
If Na transfers its 1 valence electron to Cl, Na’s second energy level becomes the valence shell, which already has 8 electrons.
Now, Na has a positive 1 charge and Cl has a negative 1 charge. But, the charge on NaCl is zero (the charges cancel each other out).
6
Na Atom
Cl Atom
Ionic Bond
Chemical Bonds: Ionic
An Ionic bond is formed when there is a transfer of electrons from a metal to a nonmetal. Compounds formed by ionic bonds are ...
The document discusses atomic structure and ions. It defines isotopes as atoms of the same element with different numbers of neutrons. The outermost electrons of an atom are involved in chemical reactions. The periodic table arranges elements by their number of outermost electrons. Noble gases have full outermost shells with 2 or 8 electrons. Atoms form ions by gaining or losing electrons to achieve stable configurations. Positively charged ions are formed when electrons are lost, and negatively charged ions are formed when electrons are gained.
An electron is a negatively charged particle that orbits the nucleus of an atom. A proton is a positively charged particle found within the nucleus. A neutron is a particle within the nucleus that has no charge. Atoms are made up of electrons orbiting a nucleus containing protons and neutrons. Elements are substances made of only one type of atom that cannot be broken down further by chemical or physical changes. Atoms of the same element have the same number of protons but can differ in the number of neutrons, forming isotopes of that element.
This document outlines key concepts about atomic structure including:
1) The structure of atoms including protons, neutrons, and electrons that make up the nucleus and electron cloud.
2) Atomic properties such as atomic number, mass number, and relative atomic mass.
3) Electron configuration, isotopes, ions, and molecules of elements and compounds.
4) Learning objectives are to describe atomic structure, state particle properties, define related terms, list uses of isotopes, and predict bonding based on structure.
1. Atoms consist of a positively charged nucleus surrounded by electrons that orbit in defined shells or energy levels.
2. The number of protons in the nucleus defines the atomic number of an element, while the total number of protons and neutrons gives the mass number.
3. Chemical properties are determined by valence electrons in the outer shell. Elements tend to gain or lose electrons to achieve a stable outer shell of 8 electrons.
The document outlines key concepts about atomic structure including the structure of atoms with protons, neutrons and electrons, atomic number and mass number, electron configuration, isotopes, ions, and molecules of elements and compounds. It also provides learning outcomes for describing atomic structure and properties as well as interpreting atomic symbols and notations.
The document outlines key learning outcomes and concepts about atomic structure, including describing the structure of atoms with atomic numbers 1 to 20, defining terms like atomic number and mass number, explaining electron configuration and outer electrons, and distinguishing between isotopes, ions, and molecules of elements and compounds. It also provides illustrations of atomic structure and examples of applying atomic structure concepts.
This document summarizes key concepts about the chemical context of life. It discusses that matter exists as elements and compounds, and the essential elements that make up living things like carbon, hydrogen, oxygen and nitrogen. It also describes the structure of atoms including subatomic particles like protons, neutrons and electrons. Electron configuration determines an element's chemical properties. Chemical bonds like covalent and ionic bonds form when atoms interact and share or transfer electrons.
This document outlines key concepts about atomic structure including:
1) The structure of atoms consists of a nucleus containing protons and neutrons surrounded by electrons. Protons are positively charged, neutrons have no charge, and electrons are negatively charged.
2) Atomic number refers to the number of protons in an atom. Mass number refers to the total number of protons and neutrons. Atomic symbols represent these numbers.
3) Electrons surround the nucleus in fixed shells. The number of electrons in each shell is limited. The arrangement of electrons is known as the electronic structure or electron configuration.
The document discusses atomic structure and subatomic particles. It explains that atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The nucleus is positively charged while electrons are negatively charged. Atoms are electrically neutral overall since the positive and negative charges balance out. Isotopes are atoms of the same element that differ in the number of neutrons. Valence electrons determine an element's chemical properties and atoms can gain or lose electrons to achieve a full outer shell, becoming ions in the process.
The document provides information about the structure of atoms. It discusses that atoms are made up of protons, neutrons and electrons. The protons and neutrons are located in the nucleus at the center, while the electrons move around the nucleus. It explains different atomic models proposed by scientists like Thomson, Rutherford and Bohr. It also discusses the distribution of electrons in shells, valency, atomic number and mass number. Isotopes and isobars are defined. In summary, the document outlines the key particles that make up an atom and the various atomic structure models developed over time.
The document provides an overview of key concepts related to the periodic table, including its organization based on electron configuration and properties of elements and ions. It explains that the periodic table arranges elements in periods and groups based on their number of protons and electrons, and that elements in the same group have similar chemical properties. It also summarizes how ions form by gaining or losing valence electrons, and how to determine the number of protons, electrons, and neutrons of elements and isotopes using atomic number and mass number.
This document provides a summary of basic chemistry concepts including:
1. Matter is anything that occupies space and has mass, and can undergo physical or chemical changes. The four main elements that make up the human body are carbon, oxygen, hydrogen, and nitrogen.
2. Atoms are the building blocks of elements and contain protons, neutrons, and electrons. The number of protons determines the element. Isotopes of elements vary in neutron number.
3. Molecules are formed by chemical bonds between two or more like atoms, while compounds contain two or more different atoms bonded together. Electron configuration and bonding allow for chemical reactions.
This document discusses ionic and metallic bonding. It explains that ions are formed when atoms gain or lose electrons to achieve stable noble gas electron configurations. Metals form cations by losing electrons while nonmetals form anions by gaining electrons. Ionic compounds contain cations and anions in ratios represented by chemical formulas. Metallic bonding occurs via delocalized valence electrons that are shared between metal atoms.
Chemical bonding involves atoms forming stable electronic configurations through gaining, losing or sharing electrons. Ionic bonds form between metals and nonmetals when electrons are transferred, while covalent bonds involve sharing electron pairs between nonmetals to achieve stable octets. Different bond types including ionic, covalent and metallic bonding can be identified based on the participating elements and electron configurations involved.
This document provides an overview of atomic structure and models of the atom. It discusses Dalton's atomic theory, subatomic particles including protons, neutrons, and electrons. Atoms are composed of a nucleus containing protons and neutrons, with electrons orbiting the nucleus. Elements differ based on their number of protons. Isotopes are versions of the same element that differ in their number of neutrons. The structure of atoms is further explained through electron configuration diagrams and quantum numbers that describe the location of electrons. Later atomic models such as the Bohr model and electron cloud model improved upon representing the structure and behavior of electrons.
Chemical bonds help determine the characteristics and properties of elements and compounds. Chemical formulas use symbols and subscripts to represent the number and type of atoms in a molecule or compound. Chemical bonds can be ionic, where atoms gain or lose electrons to form charged ions, or covalent, where atoms share or exchange electrons through electron dot diagrams.
Hello everyone, I am Dr. Ujwalkumar Trivedi, Head of Biotechnology Department at Marwadi University Rajkot. I teach Molecular Biology to the students of M.Sc. Microbiology and Biotechnology.
The current presentation talks about the formation of chemical bonds. This presentation gives insight into the formation of Ionic Bonds, Covalent Bonds and Metallic Bonds with examples.
7. Electron Dot Diagrams Shells are represented by circles and electrons are represented by dots. Example: Helium Nucleus: 2 protons, 2 neutrons 2 electrons in 1 st shell 2p 2n