Naming ionic compounds intro
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This document discusses the formation of ionic bonds between ions. Ionic bonds are electrostatic attractions between oppositely charged ions. Cations are positively charged ions formed when metals lose electrons. Anions are negatively charged ions formed when nonmetals gain electrons. Ionic bonds generally form between metallic cations and nonmetallic anions. The document provides examples of common cations and anions and identifies metals, nonmetals, and metalloids on the periodic table.
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Ion formation
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
Lewis dot structures
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
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Chapter 7 and 8 notes
This document provides an overview of ionic and covalent bonding. It discusses the formation of ions through the loss or gain of valence electrons to achieve stable electron configurations. Ionic compounds are formed between metallic and nonmetallic elements and are held together by ionic bonds between cations and anions. Molecular compounds are formed by the sharing of valence electrons between nonmetallic elements to form covalent bonds. Polar and nonpolar covalent bonds are discussed based on differences in electronegativity between bonded atoms. Hydrogen bonds that occur between polar molecules like water are also summarized. Key terms related to ionic bonding, covalent bonding, and molecular structure are defined.
Chemical Names and Formulas
This document discusses classifying and naming ionic and covalent compounds, as well as writing their formulas. It provides rules for:
- Classifying compounds as ionic or covalent based on their formula
- Naming ionic compounds using stock systems and identifying polyatomic ions
- Naming covalent compounds using prefixes to indicate the number of atoms
- Writing formulas for ionic compounds by balancing charges and for covalent compounds using prefixes
It also discusses acids, bases, and how to name and write formulas for acids based on their anion name endings.
Law of multiple proportions and law of definite proportions
The document discusses several laws related to chemical reactions and composition:
The Law of Definite Proportions states that a chemical compound always has the same proportions by mass of elements. The Law of Multiple Proportions states that when two elements form multiple compounds, the ratios of one element's masses are small whole numbers. The Law of Conservation of Mass states the total mass remains the same in a chemical reaction. Examples and practice problems demonstrate applying these laws.
Chemical Bonding
The document discusses chemical bonding and molecular structures. It explains that chemical bonding occurs through ionic bonding via the transfer of electrons between atoms, or covalent bonding via the sharing of electron pairs between atoms. It also describes molecular geometry models including VSEPR theory, which predicts the three-dimensional arrangements of atoms in molecules based on electron pair repulsion. Common molecular shapes such as linear, trigonal planar, tetrahedral and octahedral are defined.
Ion formation
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
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Ion formation
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
Lewis dot structures
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
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This document defines and provides examples of atoms, elements, molecules, and compounds. It states that atoms are the basic unit of a chemical element and are made up of protons, neutrons, and electrons. An element is made of only one type of atom, while a molecule forms when two or more atoms bond together, whether of the same or different elements. A compound contains at least two different elements bonded together. It provides examples like water (H2O) as both a molecule and compound since it contains hydrogen and oxygen atoms bonded together.
Chapter 7 and 8 notes
This document provides an overview of ionic and covalent bonding. It discusses the formation of ions through the loss or gain of valence electrons to achieve stable electron configurations. Ionic compounds are formed between metallic and nonmetallic elements and are held together by ionic bonds between cations and anions. Molecular compounds are formed by the sharing of valence electrons between nonmetallic elements to form covalent bonds. Polar and nonpolar covalent bonds are discussed based on differences in electronegativity between bonded atoms. Hydrogen bonds that occur between polar molecules like water are also summarized. Key terms related to ionic bonding, covalent bonding, and molecular structure are defined.
Chemical Names and Formulas
This document discusses classifying and naming ionic and covalent compounds, as well as writing their formulas. It provides rules for:
- Classifying compounds as ionic or covalent based on their formula
- Naming ionic compounds using stock systems and identifying polyatomic ions
- Naming covalent compounds using prefixes to indicate the number of atoms
- Writing formulas for ionic compounds by balancing charges and for covalent compounds using prefixes
It also discusses acids, bases, and how to name and write formulas for acids based on their anion name endings.
Law of multiple proportions and law of definite proportions
The document discusses several laws related to chemical reactions and composition:
The Law of Definite Proportions states that a chemical compound always has the same proportions by mass of elements. The Law of Multiple Proportions states that when two elements form multiple compounds, the ratios of one element's masses are small whole numbers. The Law of Conservation of Mass states the total mass remains the same in a chemical reaction. Examples and practice problems demonstrate applying these laws.
Chemical Bonding
The document discusses chemical bonding and molecular structures. It explains that chemical bonding occurs through ionic bonding via the transfer of electrons between atoms, or covalent bonding via the sharing of electron pairs between atoms. It also describes molecular geometry models including VSEPR theory, which predicts the three-dimensional arrangements of atoms in molecules based on electron pair repulsion. Common molecular shapes such as linear, trigonal planar, tetrahedral and octahedral are defined.
Ion formation
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Properties of Ionic compounds and Covalent Bonds
Ionic compounds:
1. Form crystals and conduct electricity when dissolved in water or molten but do not conduct in solid state.
2. Are hard, brittle, and have high melting and boiling points.
3. Are good electrical insulators.
Covalent bonds:
1. Result from the sharing of electron pairs between two atoms.
2. Occur when electron pairs are shared by atoms, as seen in single, double and triple bonds between similar or dissimilar atoms.
3. Differ from ionic bonds which form through the transfer of electrons between metals and nonmetals.
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Lecture 8.1- Ionic vs. Covalent
The document provides information about ionic and covalent (molecular) bonding:
- Ionic bonds occur between metals and non-metals and involve the transfer of electrons. Covalent bonds occur between two non-metals and involve the sharing of electrons.
- Ionic compounds have high melting and boiling points and conduct electricity when melted or dissolved. Molecular compounds have lower melting and boiling points and do not conduct electricity.
- Ionic compounds exist as crystal lattices of ions, while molecular compounds exist as distinct molecules made of two or more nonmetal atoms bonded together.
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Chemical bonding
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between oppositely charged ions, such as between sodium and chlorine atoms where sodium loses an electron to become positively charged and chlorine gains an electron to become negatively charged. Covalent bonds form when atoms share electrons, such as in water where oxygen and hydrogen share electron pairs. Metallic bonds form by the attraction of free-floating electrons within a lattice of positive metal ions.
Ionic bonding
Ionic bonding occurs when atoms of metals and non-metals combine to form ionic compounds. Atoms of metals will donate electrons to form cations, while atoms of non-metals will accept electrons to form anions. This transfer of electrons allows the atoms to achieve stable electron configurations similar to noble gases. Common examples are sodium chloride, which forms when sodium donates an electron to chlorine, and magnesium oxide, which forms when magnesium donates two electrons to oxygen. The chemical formulas of ionic compounds are written to balance the charges of the cation and anion.
Ionic Compounds
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.
Chemical bonds.ppt
Atoms form bonds by gaining, losing, or sharing electrons to attain a stable electron configuration with 8 valence electrons, known as an octet. Ionic bonds form when atoms transfer electrons to become ions with opposite charges that are attracted to each other. Covalent bonds form when atoms share electrons to attain a full outer shell. Common diatomic molecules that form through covalent bonding include hydrogen (H2), oxygen (O2), nitrogen (N2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2). Ionic bonds typically form between metals and nonmetals, while covalent bonds form between two nonmetals.
Ionic bonding
Ionic bonds form when a metal transfers an electron to a nonmetal, giving each atom an octet of electrons. For example, sodium loses an electron to form Na+ while chlorine gains that electron to form Cl-. The resulting ions are held together by electrostatic attraction to form an ionic compound, sodium chloride (NaCl). NaCl forms a crystalline lattice structure where the Na+ and Cl- ions are arranged in a repeating pattern. Ionic compounds have properties like high melting points, conductivity when molten or dissolved, and solubility in water.
Metallic bonds
Metals form metallic bonds when their valence electrons are released and move freely around the positively charged metal ions, creating a "sea of electrons". This sea of delocalized electrons is what gives metals their characteristic properties like malleability, ductility, luster, and high electrical and thermal conductivity. Alloys are mixtures of metals that are generally stronger yet less reactive than their pure metal components due to the metallic bonding between different kinds of metal atoms and ions.
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Here are the key points about homogeneous and heterogeneous mixtures:
- Homogeneous mixtures have uniform composition and appearance throughout. Common examples include solutions.
- Heterogeneous mixtures have visibly distinct parts that can be seen without using a microscope. The substances do not dissolve or blend uniformly.
- Homogeneous mixtures are examples of single phase systems while heterogeneous mixtures contain two or more phases (solid, liquid, gas).
- Sugar solution is an example of a homogeneous mixture where sugar is dissolved uniformly throughout the water. Water and oil is an example of a heterogeneous mixture since the substances do not dissolve in each other and remain as separate visible layers.
The key difference is that homogeneous mixtures appear uniform while heterogeneous mixtures have distinct parts
Ions cations and anions
Ions are atoms that have gained or lost electrons, giving them an electrical charge. Atoms that lose electrons become positively charged cations, while atoms that gain electrons become negatively charged anions. The number of protons and neutrons remain the same in an ion, only the number of electrons changes. Ionic bonding occurs through the transfer of electrons from one atom to another, while covalent bonding involves the sharing of electron pairs between two atoms. Sodium chloride is an example of ionic bonding through electron transfer, while an oxygen molecule is held together by covalent bonding from shared electron pairs.
FORMATION OF COVALENT BOND
This document discusses the formation of covalent bonds. It defines covalent bonds as the sharing of electron pairs between nonmetal atoms. There are three types of covalent bonds: single, double, and triple bonds which are formed by the sharing of one, two, or three electron pairs respectively. Examples of bond formation in H2, O2, and N2 molecules are provided to illustrate single, double, and triple bonds. The key differences between ionic and covalent bonds are that ionic bonds involve electron transfer between metals and nonmetals while covalent bonds involve electron sharing between nonmetals.
Naming ionic compounds cations anions
This document discusses naming ionic compounds by first naming the cation and anion components. It provides rules for naming main group and transition metal cations, such as naming sodium as the "sodium cation" and copper as the "copper (II) cation". It also provides rules for naming anions by taking the root of the element name and adding "-ide", such as naming chloride and bromide anions. Examples and practice problems are given to demonstrate applying these rules to name common cations and anions.
Valence Electrons
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.
Molecular Compounds
Molecular compounds are formed when atoms of two or more different non-metals combine through covalent bonds. Covalent bonds involve the sharing of electron pairs between atoms. Molecular compounds have properties such as being soft, having low melting points, and not conducting electricity. The naming of molecular compounds involves naming the elements present and indicating the number of atoms through prefixes.
Ionic bonding
The document discusses the determination of lattice energy of ionic compounds using the Born-Haber cycle. It explains that the lattice energy of sodium chloride can be determined experimentally by considering its formation through two different methods. Method 1 is the direct combination of solid sodium and gaseous chlorine to form solid sodium chloride. Method 2 involves 5 steps including sublimation, dissociation, ionization, and combining to form ions and the ionic solid. Using Hess's law, the lattice energy is calculated by equating the enthalpy change between the two methods. For sodium chloride, the calculated lattice energy is -773.95 kJ/mol.
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Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Properties of Ionic compounds and Covalent Bonds
Ionic compounds:
1. Form crystals and conduct electricity when dissolved in water or molten but do not conduct in solid state.
2. Are hard, brittle, and have high melting and boiling points.
3. Are good electrical insulators.
Covalent bonds:
1. Result from the sharing of electron pairs between two atoms.
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3. Differ from ionic bonds which form through the transfer of electrons between metals and nonmetals.
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Lecture 8.1- Ionic vs. Covalent
The document provides information about ionic and covalent (molecular) bonding:
- Ionic bonds occur between metals and non-metals and involve the transfer of electrons. Covalent bonds occur between two non-metals and involve the sharing of electrons.
- Ionic compounds have high melting and boiling points and conduct electricity when melted or dissolved. Molecular compounds have lower melting and boiling points and do not conduct electricity.
- Ionic compounds exist as crystal lattices of ions, while molecular compounds exist as distinct molecules made of two or more nonmetal atoms bonded together.
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Ionic bonding
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.
Chemical bonding
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between oppositely charged ions, such as between sodium and chlorine atoms where sodium loses an electron to become positively charged and chlorine gains an electron to become negatively charged. Covalent bonds form when atoms share electrons, such as in water where oxygen and hydrogen share electron pairs. Metallic bonds form by the attraction of free-floating electrons within a lattice of positive metal ions.
Ionic bonding
Ionic bonding occurs when atoms of metals and non-metals combine to form ionic compounds. Atoms of metals will donate electrons to form cations, while atoms of non-metals will accept electrons to form anions. This transfer of electrons allows the atoms to achieve stable electron configurations similar to noble gases. Common examples are sodium chloride, which forms when sodium donates an electron to chlorine, and magnesium oxide, which forms when magnesium donates two electrons to oxygen. The chemical formulas of ionic compounds are written to balance the charges of the cation and anion.
Ionic Compounds
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.
Chemical bonds.ppt
Atoms form bonds by gaining, losing, or sharing electrons to attain a stable electron configuration with 8 valence electrons, known as an octet. Ionic bonds form when atoms transfer electrons to become ions with opposite charges that are attracted to each other. Covalent bonds form when atoms share electrons to attain a full outer shell. Common diatomic molecules that form through covalent bonding include hydrogen (H2), oxygen (O2), nitrogen (N2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2). Ionic bonds typically form between metals and nonmetals, while covalent bonds form between two nonmetals.
Ionic bonding
Ionic bonds form when a metal transfers an electron to a nonmetal, giving each atom an octet of electrons. For example, sodium loses an electron to form Na+ while chlorine gains that electron to form Cl-. The resulting ions are held together by electrostatic attraction to form an ionic compound, sodium chloride (NaCl). NaCl forms a crystalline lattice structure where the Na+ and Cl- ions are arranged in a repeating pattern. Ionic compounds have properties like high melting points, conductivity when molten or dissolved, and solubility in water.
Metallic bonds
Metals form metallic bonds when their valence electrons are released and move freely around the positively charged metal ions, creating a "sea of electrons". This sea of delocalized electrons is what gives metals their characteristic properties like malleability, ductility, luster, and high electrical and thermal conductivity. Alloys are mixtures of metals that are generally stronger yet less reactive than their pure metal components due to the metallic bonding between different kinds of metal atoms and ions.
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Here are the key points about homogeneous and heterogeneous mixtures:
- Homogeneous mixtures have uniform composition and appearance throughout. Common examples include solutions.
- Heterogeneous mixtures have visibly distinct parts that can be seen without using a microscope. The substances do not dissolve or blend uniformly.
- Homogeneous mixtures are examples of single phase systems while heterogeneous mixtures contain two or more phases (solid, liquid, gas).
- Sugar solution is an example of a homogeneous mixture where sugar is dissolved uniformly throughout the water. Water and oil is an example of a heterogeneous mixture since the substances do not dissolve in each other and remain as separate visible layers.
The key difference is that homogeneous mixtures appear uniform while heterogeneous mixtures have distinct parts
Ions cations and anions
Ions are atoms that have gained or lost electrons, giving them an electrical charge. Atoms that lose electrons become positively charged cations, while atoms that gain electrons become negatively charged anions. The number of protons and neutrons remain the same in an ion, only the number of electrons changes. Ionic bonding occurs through the transfer of electrons from one atom to another, while covalent bonding involves the sharing of electron pairs between two atoms. Sodium chloride is an example of ionic bonding through electron transfer, while an oxygen molecule is held together by covalent bonding from shared electron pairs.
FORMATION OF COVALENT BOND
This document discusses the formation of covalent bonds. It defines covalent bonds as the sharing of electron pairs between nonmetal atoms. There are three types of covalent bonds: single, double, and triple bonds which are formed by the sharing of one, two, or three electron pairs respectively. Examples of bond formation in H2, O2, and N2 molecules are provided to illustrate single, double, and triple bonds. The key differences between ionic and covalent bonds are that ionic bonds involve electron transfer between metals and nonmetals while covalent bonds involve electron sharing between nonmetals.
Naming ionic compounds cations anions
This document discusses naming ionic compounds by first naming the cation and anion components. It provides rules for naming main group and transition metal cations, such as naming sodium as the "sodium cation" and copper as the "copper (II) cation". It also provides rules for naming anions by taking the root of the element name and adding "-ide", such as naming chloride and bromide anions. Examples and practice problems are given to demonstrate applying these rules to name common cations and anions.
Valence Electrons
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.
Molecular Compounds
Molecular compounds are formed when atoms of two or more different non-metals combine through covalent bonds. Covalent bonds involve the sharing of electron pairs between atoms. Molecular compounds have properties such as being soft, having low melting points, and not conducting electricity. The naming of molecular compounds involves naming the elements present and indicating the number of atoms through prefixes.
Ionic bonding
The document discusses the determination of lattice energy of ionic compounds using the Born-Haber cycle. It explains that the lattice energy of sodium chloride can be determined experimentally by considering its formation through two different methods. Method 1 is the direct combination of solid sodium and gaseous chlorine to form solid sodium chloride. Method 2 involves 5 steps including sublimation, dissociation, ionization, and combining to form ions and the ionic solid. Using Hess's law, the lattice energy is calculated by equating the enthalpy change between the two methods. For sodium chloride, the calculated lattice energy is -773.95 kJ/mol.
What are groups and periods?
This document is a lesson on groups and periods in the periodic table. It defines periods as rows from left to right, and groups as columns from top to bottom. Elements in the same group have similar properties because they have the same number of valence electrons. The lesson discusses special metal and nonmetal groups, including alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. It provides examples of elements in each group and their properties. The document concludes with practice questions for students.
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Properties of Compounds - Ionic, Covalent and Metallic
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This document provides an overview of key concepts related to gases, including:
- The properties of ideal gases and units of pressure like pascals and atmospheres.
- Gas laws including Boyle's, Charles', Gay-Lussac's, Avogadro's, and the ideal gas law.
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Naming ionic compounds writing emp formulas
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
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Naming ionic compounds intro
- 1. Naming Ionic Compounds Part 1: Cations, Anions, and Ionic Bonds By Shawn P. Shields, Ph.D. This work is licensed by Shawn P. Shields-Maxwell under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License.
- 2. What are Ionic Bonds? Ionic bonds are formed by electrostatic attractions between oppositely-charged ions Cations are formed when an atom loses electrons to form a positively-charged ion. (Xn+) Anions are formed when an atom gains electrons to form a negatively-charged ion. (Xn) Ionic bonds are generally formed between metals and nonmetals. + Recall:
- 3. Recall: Identifying Metals and Nonmetals on the Periodic Table
- 4. Main Group Metals Alkali (group 1) and alkaline earth (group 2) metals Other main group metals Hydrogen (H) is considered a nonmetal, even though it is in group 1. H usually forms H+ ions.
- 5. Main Group Metals Metals form cations (positively-charged ions). Examples: Sodium cation (Na+) in Group 1 Magnesium cation (Mg2+) in Group 2 Aluminum cation (Al3+) in Group 3 Main group metal cations have a positive charge equal to the group number. Hydrogen (H) is considered a nonmetal, even though it is in group 1. H usually forms H+ ions, except when bonded to metals.
- 6. Transition Metals Transition metals are located in the center portion of the periodic table (also called the “d-block”)
- 7. Transition Metals Transition metals form cations (positively-charged ions). Most have more than one possible charge for the cation. Examples: Iron: Fe2+ and Fe3+ Copper: Cu+ and Cu2+ Gold: Au+ and Au3+
- 8. Nonmetals Nonmetals are generally found on the right hand side of the table
- 9. Nonmetals in Ionic Compounds Nonmetals generally form anions (negatively- charged ions) when in ionic compounds. Examples: Chloride anion (Cl) Oxide anion (O2) Sulfide anion (S2) Nonmetals form covalent, as opposed to ionic, bonds when bonded to other nonmetals. Noble gases (group 8) do not form ions.
- 10. Identifying Metals and Nonmetals on the Periodic Table Metalloids
- 11. Metalloids Metalloids (generally) form covalent as opposed to ionic bonds in compounds. In particular, compounds composed from a nonmetal and a metalloid contain covalent bonds.
- 12. Summary Metals form cations in ionic compounds. Cations are positively-charged ions. When a cation is formed, the atom loses electrons. Nonmetals form anions in ionic compounds. Anions are negatively-charged ions. When an anion is formed, the atom gains electrons. Ionic compounds form between metals and nonmetals. An ionic bond is an electrostatic attraction between oppositely-charged particles (ions).