Ionic bonding revision
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PB_HThe document discusses ionic bonding. It explains that sodium has 11 protons, 11 electrons, and a 0 charge. Chlorine has 17 protons, 17 electrons, and a 0 charge. For sodium to have a full outer shell, it loses 1 electron and gains a +1 charge. For chlorine to have a full outer shell, it gains 1 electron and gains a -1 charge. This creates sodium and chloride ions, Na+ and Cl-, which are attracted to each other due to their opposite charges. When they bond, they form an ionic compound, sodium chloride, with a repeating pattern that gives it a cubic crystal structure.
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Ionic compounds are formed from a cation and an anion. Opposite charges attract the ions together in an ionic bond. Ions transfer electrons to achieve stable noble gas electron configurations. Ionic compounds have crystalline structures where ions are arranged in repeating patterns. The ions are strongly bonded and give ionic solids properties like brittleness and ability to conduct electricity when molten or dissolved in water.
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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 crystallizes into a repeating pattern where Na+ and Cl- ions alternate in a crystal lattice. Ionic compounds conduct electricity when molten or dissolved due to the movement of ions.
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Ionic compounds are formed from a cation and an anion. Opposite charges attract the ions together in an ionic bond. Ions transfer electrons to achieve stable noble gas electron configurations. Ionic compounds have crystalline structures where ions are arranged in repeating patterns. The ions are strongly bonded and give ionic solids properties like brittleness and ability to conduct electricity when molten or dissolved in water.
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Chemical bonding covalent
1) Covalent bonding occurs when two nonmetal atoms share electrons in their outer shells to achieve a stable full outer shell.
2) Atoms that cannot gain or lose electrons, like carbon, must share electrons through covalent bonds rather than forming ions. They share electrons tightly in molecular compounds.
3) Double and triple covalent bonds form when two or three pairs of electrons are shared between two atoms, as seen in carbon dioxide and nitrogen molecules.
Chem matters ch6_ionic_bond
1) Noble gases are unreactive because their outer electron shells are full, giving them a stable configuration.
2) Atoms form ions to achieve a full outer shell like noble gases. Metals form cations by losing electrons, and non-metals form anions by gaining electrons.
3) Ionic bonds form when oppositely charged ions are attracted to each other, such as sodium and chloride ions forming sodium chloride. The chemical formula shows the ratio of ions.
General Chemistry at the University of Oklahoma Exam 2
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
CH.6 (PART II) - PROPERTIES of Ionic Compounds ppt. (2022).pptx
This document discusses the structure and properties of ionic compounds. It begins by explaining that ionic compounds are formed through the electrostatic attraction between oppositely charged ions. The ions form a crystalline lattice structure held together by strong ionic bonds. This lattice structure results in ionic compounds having high melting points, hardness, and brittleness. The document then discusses how ionic bonding occurs through the transfer of electrons between metals and nonmetals. It provides examples of writing chemical formulas and naming ionic compounds based on their ion charges.
Unit 3 3 ions
This document introduces ions to students. It defines an ion as a charged particle formed when an atom gains or loses electrons. Cations have a positive charge from losing electrons, and anions have a negative charge from gaining electrons. Examples show sodium forming Na+ by losing an electron, and chlorine forming Cl- by gaining an electron. Common ions can be predicted based on an element's location in the periodic table. Groups 1 and 2 typically form cations by losing electrons, while groups 15-17 typically form anions by gaining electrons.
chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
bonding_regents_chem.ppt
This document defines chemical bonding and describes the three main types of bonds: metallic, ionic, and covalent. Metallic bonds form a crystalline lattice structure with freely moving electrons. Ionic bonds form when ions with opposite charges are attracted to each other via electrostatic forces. Covalent bonds form when atoms share electrons to achieve stable electron configurations. The type of bonding determines various physical properties like melting point, hardness, and conductivity.
Chemical bonding part 2
The document discusses different types of chemical bonding including ionic bonds, covalent bonds, hydrogen bonds, and metallic bonds. Ionic bonds form when a metal transfers electrons to a nonmetal to form positive and negative ions that are attracted via electrostatic forces. Covalent bonds form when two nonmetals share electrons to achieve a full outer shell. Hydrogen bonds are strong dipole interactions between a hydrogen atom covalently bonded to a fluorine, oxygen, or nitrogen and another polar molecule. Metallic bonds involve free-floating valence electrons that allow metal atoms to slide past one another and conduct electricity.
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Ionic bonding revision
- 2. How can atoms turn into ions? Sodium 11 0 Electrons = Protons = 11 Charge = Chlorine 17 0 Electrons = Protons = 17 Charge =
- 3. How can atoms turn into ions? Sodium 11 0 Electrons = Protons = 11 Charge = Chlorine 17 0 Electrons = Protons = 17 Charge = 1 electron in outer shell
- 4. How can atoms turn into ions? Sodium 11 0 Electrons = Protons = 11 Charge = Chlorine 17 0 Electrons = Protons = 17 Charge = 1 electron needed to gain a full outer shell
- 5. How can atoms turn into ions? Sodium 11 +1 Electrons = Protons = 11 Charge = Chlorine 17 -1 Electrons = Protons = 17 Charge = The electron moves
- 6. How can atoms turn into ions? Sodium 11Electrons = Protons = 11 Charge = Chlorine 17Electrons = Protons = 17 Charge = This creates two charges ions + - +1 -1
- 7. • Write down the rules for working out the formula of an ionic compound? What to do…
- 8. • Did you get the following rules for working out the formula of an ionic compound? What to do…
- 9. What to do… 1. Identify the number of electrons in the outer shell • Did you get the following rules for working out the formula of an ionic compound?
- 10. What to do… 1. Identify the number of electrons in the outer shell 2. Establish if the atom will loose or gain electrons (and how many) to gain full shells • Did you get the following rules for working out the formula of an ionic compound?
- 11. What to do… 1. Identify the number of electrons in the outer shell 2. Establish if the atom will loose or gain electrons (and how many) to gain full shells 3. Balance the charges on positive and negative ions to make it neutral overall • Did you get the following rules for working out the formula of an ionic compound?
- 12. What happens when ions have formed?
- 13. A sodium chloride crystal is made up of millions of Na+ and Cl− ions arranged in a regular pattern. Crystals of sodium chloride The regular pattern is responsible for the cubic shape of all sodium chloride crystals.
- 14. When sodium burns in chlorine . . . chlorine hot sodium . . . Na+ and Cl− ions are formed.
- 15. • Oppositely charged ions attract each other. • Each ion attracts oppositely charged ions from all directions. • Each of these ions in turn attracts more ions. • A giant ionic structure made up of millions of ions is built up and forms a sodium chloride crystal.
- 16. What happens when NaCl is heated until it melts? heat • At the melting point, the regular arrangement of ions is broken down and the ions become free to move. • Although the ions are still close together, they can move independently, so molten NaCl conducts electricity.
- 17. Liquid water consists of H2O molecules that are close together but moving randomly. water molecule What happens when NaCl dissolves in water?
- 18. c + • When NaCl is added to water, the ions are pulled off the structure, and they become free to move in the water. • The ions can move independently, so a solution of NaCl in water conducts electricity.