BONDS AND LEWIS STRUCTURES
... considered to be nonpolar covalent and the electron sharing is more or less equal. If the difference is more than 0.5 but less than 2.1, the bond is polar covalent, which means that the sharing is unequal. If the difference is greater than 2.1, the bond is considered to be ionic, and the bonding ele ...
... considered to be nonpolar covalent and the electron sharing is more or less equal. If the difference is more than 0.5 but less than 2.1, the bond is polar covalent, which means that the sharing is unequal. If the difference is greater than 2.1, the bond is considered to be ionic, and the bonding ele ...
Ang. bindningstyper och elektronegativitet
... A coordinate covalent bond is one where both bonding electrons are from one of the atoms involved in the bond. These bonds give rise to Lewis acids and bases. The electrons are shared roughly equally between the atoms in contrast to ionic bonding. Such bonding occurs in molecules such as the ammoniu ...
... A coordinate covalent bond is one where both bonding electrons are from one of the atoms involved in the bond. These bonds give rise to Lewis acids and bases. The electrons are shared roughly equally between the atoms in contrast to ionic bonding. Such bonding occurs in molecules such as the ammoniu ...
Basic Chemistry Notes II
... 2. Have a negative charge 3. Valence electrons – outermost electron shell. Most important electrons because they determine bonding/reactivity of atom. ...
... 2. Have a negative charge 3. Valence electrons – outermost electron shell. Most important electrons because they determine bonding/reactivity of atom. ...
Bonding - Graham ISD
... Atoms combine when the compound formed id more stable than the separate atoms. The only group that seldom forms compounds is the noble gases (group 18). This is true because compounds of these atoms are almost always less stable than the original atom. Atoms with a partially stable outer energy leve ...
... Atoms combine when the compound formed id more stable than the separate atoms. The only group that seldom forms compounds is the noble gases (group 18). This is true because compounds of these atoms are almost always less stable than the original atom. Atoms with a partially stable outer energy leve ...
Chapter 12: Basic Review Worksheet
... 1. In general, what do we mean by a chemical bond? Name the principal types of chemical bonds. 2. What do we mean by ionic bonding? Give an example of a substance whose particles are held together by ionic bonding. 3. What do we mean by covalent bonding and polar covalent bonding? How are these two ...
... 1. In general, what do we mean by a chemical bond? Name the principal types of chemical bonds. 2. What do we mean by ionic bonding? Give an example of a substance whose particles are held together by ionic bonding. 3. What do we mean by covalent bonding and polar covalent bonding? How are these two ...
Learning Standards vocab chemical basis and molecules of life 09
... formed (e.g., sodium atoms lose an electron and chlorine atoms gain an electron, then the charged ions are attracted to each other and form bonds). Explain the meaning of a chemical formula for an ionic array (e.g., NaCl). Give examples to illustrate that molecules are groups of two or more atom ...
... formed (e.g., sodium atoms lose an electron and chlorine atoms gain an electron, then the charged ions are attracted to each other and form bonds). Explain the meaning of a chemical formula for an ionic array (e.g., NaCl). Give examples to illustrate that molecules are groups of two or more atom ...
Word - chemmybear.com
... Atoms tend to lose, gain, or ___________ electrons to complete their valence shells. When a chlorine atom gains an electron, it fills its valence shell forming a negative chloride________. Whenever ionic solids are formed, __________ is involved. An ionic material is composed of positive ions bonded ...
... Atoms tend to lose, gain, or ___________ electrons to complete their valence shells. When a chlorine atom gains an electron, it fills its valence shell forming a negative chloride________. Whenever ionic solids are formed, __________ is involved. An ionic material is composed of positive ions bonded ...
Student Learning Map
... What is the VSEPR theory and how is it used to determine the shape (molecular geometry) of a molecule? ...
... What is the VSEPR theory and how is it used to determine the shape (molecular geometry) of a molecule? ...
Module 8 - Brookville Local Schools
... Part of the Chemistry For Dummies Cheat Sheet In bonding, atoms lose, gain, or share electrons in order to have the same number of electrons as the noble gas that's nearest on the periodic table. Ionic, covalent, and metallic bonds are formed by combinations of metals and nonmetals. Metal + nonmet ...
... Part of the Chemistry For Dummies Cheat Sheet In bonding, atoms lose, gain, or share electrons in order to have the same number of electrons as the noble gas that's nearest on the periodic table. Ionic, covalent, and metallic bonds are formed by combinations of metals and nonmetals. Metal + nonmet ...
2.1 The Nature of Matter - Sonoma Valley High School
... Some elements have isotopes, with different #s of neutrons and different mass. All isotopes of an element have the same chemical properties b/c their electrons are the same. ...
... Some elements have isotopes, with different #s of neutrons and different mass. All isotopes of an element have the same chemical properties b/c their electrons are the same. ...
Types of Bonding Summary
... small EN difference (usually two nonmetals) Leads to separate molecules with specific shapes or to extended networks ...
... small EN difference (usually two nonmetals) Leads to separate molecules with specific shapes or to extended networks ...
Chapter 2 - Speedway High School
... • Potential energy is the energy that matter has because of its location or structure • electron shell ...
... • Potential energy is the energy that matter has because of its location or structure • electron shell ...
Chapter 6: Chemical Bonding
... • We will state the octet rule. • We will see how to write Lewis structures. • We will explain why people use resonance structures. ...
... • We will state the octet rule. • We will see how to write Lewis structures. • We will explain why people use resonance structures. ...
Chapter 8: Chemical Reactions and Physical Changes
... • Mass number: total protons and neutrons in an atom’s nucleus • Atomic mass: the average mass of a sample of atoms of that element found in nature • Periodic table: chart that arranges elements by atomic number into rows and columns according to similarities in their properties ...
... • Mass number: total protons and neutrons in an atom’s nucleus • Atomic mass: the average mass of a sample of atoms of that element found in nature • Periodic table: chart that arranges elements by atomic number into rows and columns according to similarities in their properties ...
Word - chemmybear.com
... Lattice: a repeating pattern, like a lattice-work fence. In solids, it is a repeating pattern of atoms. All solids are made up of a lattice. The points of the lattice are different in different types of solids. ...
... Lattice: a repeating pattern, like a lattice-work fence. In solids, it is a repeating pattern of atoms. All solids are made up of a lattice. The points of the lattice are different in different types of solids. ...
First Semester Final - Review Questions
... 1. What is atomic number? 2. How does increasing the atomic number affect the identity of an atom? 3. What is atomic mass? What two subatomic particles make up the majority of an atom’s mass? 4. Describe the gold foil experiment. What was the important discovery in that experiment? 5. Where are the ...
... 1. What is atomic number? 2. How does increasing the atomic number affect the identity of an atom? 3. What is atomic mass? What two subatomic particles make up the majority of an atom’s mass? 4. Describe the gold foil experiment. What was the important discovery in that experiment? 5. Where are the ...
Covalent Bonds
... 3. If central atom is not yet surrounded by 4 electron pairs or does not form an octet, convert one or more of the lone pairs from a terminal atom into double or triple bonds. This will only happen with C, N, O, P, or S. ...
... 3. If central atom is not yet surrounded by 4 electron pairs or does not form an octet, convert one or more of the lone pairs from a terminal atom into double or triple bonds. This will only happen with C, N, O, P, or S. ...
Ch 6 Jeopardy Review
... In these bonds valence electrons are able to freely move between a cation lattice. ...
... In these bonds valence electrons are able to freely move between a cation lattice. ...
chemical bond
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
2.5 Chemical Bonding - Lighthouse Christian Academy
... • Another type of bonding occurs when non-metals ‘share’ their valence e with other non-metals to complete their valence shells. • This bonding is called covalent bonding and builds atoms into covalent or molecular compounds. • Therefore, in covalent bonding, a sharing of valence electrons occurs ( ...
... • Another type of bonding occurs when non-metals ‘share’ their valence e with other non-metals to complete their valence shells. • This bonding is called covalent bonding and builds atoms into covalent or molecular compounds. • Therefore, in covalent bonding, a sharing of valence electrons occurs ( ...
Chemical bond
A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are ""strong bonds"" such as covalent or ionic bonds and ""weak bonds"" such as Dipole-dipole interaction, the London dispersion force and hydrogen bonding.Since opposite charges attract via a simple electromagnetic force, the negatively charged electrons that are orbiting the nucleus and the positively charged protons in the nucleus attract each other. An electron positioned between two nuclei will be attracted to both of them, and the nuclei will be attracted toward electrons in this position. This attraction constitutes the chemical bond. Due to the matter wave nature of electrons and their smaller mass, they must occupy a much larger amount of volume compared with the nuclei, and this volume occupied by the electrons keeps the atomic nuclei relatively far apart, as compared with the size of the nuclei themselves. This phenomenon limits the distance between nuclei and atoms in a bond.In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms. The atoms in molecules, crystals, metals and diatomic gases—indeed most of the physical environment around us—are held together by chemical bonds, which dictate the structure and the bulk properties of matter.All bonds can be explained by quantum theory, but, in practice, simplification rules allow chemists to predict the strength, directionality, and polarity of bonds. The octet rule and VSEPR theory are two examples. More sophisticated theories are valence bond theory which includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory. Electrostatics are used to describe bond polarities and the effects they have on chemical substances.
