Bonds
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A bond is formed when two or more atoms join together through sharing or exchanging electrons to achieve stability. A molecule is two or more bonded atoms, and a substance can be either a pure element or compound made of two or more elements. There are two main types of bonds: covalent bonds formed by sharing electrons between nonmetals and ionic bonds formed by a transfer of electrons between a metal and nonmetal. The periodic table arranges elements and can provide information about their valence electrons and reactivity through bonding properties.
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This document defines key terms related to chemical bonds and discusses how atoms bond to achieve stable electron configurations. It explains that atoms form ions by gaining or losing electrons to achieve a full outer electron shell like noble gases. Metals typically lose electrons to form positive ions while nonmetals gain electrons to form negative ions. These oppositely charged ions then form ionic bonds. The document also describes how nonmetal atoms can form covalent bonds by sharing electrons to achieve full outer shells. Polyatomic ions, which are groups of bonded atoms that act as a single unit, are presented and examples are given of how they form ionic bonds with metals through electron transfer.
Chemical Bonds
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.
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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.
Chemistry form 4 ionic bond
It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
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.
Chemistry - Chp 8 - Covalent Bonding - PowerPoint
The document summarizes key concepts about covalent bonding from a chemistry textbook chapter:
1) Covalent bonds form when two nonmetal atoms share one or more pairs of electrons to achieve a noble gas configuration, forming molecules like H2, O2, and CO2.
2) Molecular compounds formed by covalent bonds tend to have lower melting and boiling points than ionic compounds due to the weaker nature of the covalent bond.
3) Electron dot structures and Lewis diagrams are used to represent how atoms share electrons to form single, double or triple covalent bonds in molecules like H2O and NH3.
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Ionic bonding occurs between metals and nonmetals due to their differences in electronegativity. Metals have relatively low ionization energies and lose electrons to form cations, while nonmetals have high electronegativity and gain electrons to form anions. Oppositely charged ions are then attracted through electrostatic forces to form an ionic compound.
ionic bond
1) Atoms are made up of electrons, protons and neutrons. Electrons occupy electron shells and determine how an atom bonds with other atoms.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, giving them opposing charges. For example, sodium (Na) transfers an electron to chlorine (Cl), forming sodium ion (Na+) and chloride ion (Cl-).
3) Covalent bonds form when atoms share electrons to fill their outer electron shells in a stable configuration.
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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.
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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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It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
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2) Molecular compounds formed by covalent bonds tend to have lower melting and boiling points than ionic compounds due to the weaker nature of the covalent bond.
3) Electron dot structures and Lewis diagrams are used to represent how atoms share electrons to form single, double or triple covalent bonds in molecules like H2O and NH3.
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Ionic bonding occurs between metals and nonmetals due to their differences in electronegativity. Metals have relatively low ionization energies and lose electrons to form cations, while nonmetals have high electronegativity and gain electrons to form anions. Oppositely charged ions are then attracted through electrostatic forces to form an ionic compound.
ionic bond
1) Atoms are made up of electrons, protons and neutrons. Electrons occupy electron shells and determine how an atom bonds with other atoms.
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This document provides an overview of different types of chemical bonds: ionic bonds, covalent bonds, metallic bonds, and hydrogen bonds. Ionic bonds form between metals and nonmetals when atoms gain or lose electrons to become ions. Covalent bonds form when atoms share electron pairs, including both polar and nonpolar variations. Metallic bonds occur between packed metal atoms where delocalized electrons move freely between nuclei. Hydrogen bonds are dipole-dipole attractions between hydrogen atoms covalently bonded to electronegative atoms and other electronegative atoms. Examples of each bond type are given.
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This document provides information on various chemistry concepts including acids and salts, redox reactions, atomic structure and bonding, and periodic trends. It defines several acids and their molecular formulas. It describes redox reactions involving acids and bases. It also defines ionization energy, electron configuration, ionic bonding, covalent bonding and metallic bonding. Finally, it discusses factors that influence ionization energy and melting/boiling points across periods 2 and 3 based on atomic structure and bonding type.
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1) Atoms are the smallest units that make up matter and consist of protons, neutrons and electrons. Electrons orbit the nucleus in shells.
2) There are two main types of bonds between atoms - ionic bonds which involve transfer of electrons between metals and non-metals, and covalent bonds which involve sharing of electrons between non-metals.
3) Isotopes are atoms of the same element that have different numbers of neutrons, giving them different masses but the same chemical properties. Radioactive isotopes are unstable and decay over time.
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This document discusses the structure and composition of matter. It explains that all matter is made up of elements, which are composed of atoms. Atoms contain protons, neutrons, and electrons. Elements can bond together through ionic bonds, covalent bonds, or hydrogen bonds to form molecules or compounds. Some important compounds are electrolytes, acids, bases, and salts. Chemical reactions cause bonds to form or break as atoms rearrange. The human body relies on many chemical processes and requires maintaining a narrow pH range in the blood for survival.
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This document defines the three states of matter - solids, liquids, and gases. It explains that solids have particles that barely move and hold a defined shape, liquids have particles that flow freely but maintain a constant volume, and gases have particles that have no defined volume or shape and move very quickly. The document also notes that all states of matter are made up of particles that move at different speeds depending on whether they are a solid, liquid, or gas.
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Motion refers to the change in an object's position or location over time. Kinematics is the study of motion without regard to forces or energies. An object is considered in motion if its position changes relative to a reference point.
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This document provides information on chemistry topics including the structure of matter, states of matter, classifying substances, physical and chemical properties, and changes in matter. It defines key terms like elements, atoms, the periodic table, and reactivity. Chemistry is the study of matter and its changes through chemical and physical transformations.
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Bonds
- 1. Bonds By Regina López and Andrea Herrera
- 2. What is a bond? A bond is when two or more atoms are joined together to reach chemical stability.
- 3. What are molecules? A molecule is a combination of two or more atoms.
- 4. What is a substance? Substance = matter
- 5. Pure substances Elements: Na, C, K, N, Ne. Compounds: H2O, O2, CH4, C2H6
- 6. Not Pure Substances Homogeneous: salt water, gatorade, pepto bismol, coffee. Heterogeneous: pozole, Chapala lake, salad, milk and cereal.
- 7. What is a compound? A compound is any substance formed when two or more elements are bonded.
- 8. Covalent Bonds A covalent bond is formed between two nonmetals. In a covalent bond the electrons are shared.
- 9. Covalent Bonds Covalent bonds include diatomic molecules of some gases.
- 10. Ion When an atom gets a charge by either loosing or gaining electrons. If it looses electrons it will become a positive ion and if it gains it will become a negative ion.
- 11. Ionic Bonds Ionic bonds are formed between one metal and one nonmetal. In ionic bonds there is a gain and loss of electrons(The metal looses and the nonmetal gains). Debatable if they are stronger
- 12. Ionic bonds
- 13. Polyatomic ions A polyatomic ion is a bond between two or more atoms with a charge. They are formed by a covalent bond and it can make ionic bonds.
- 14. Polyatomic ions In a polyatomic ion the resulting number of electrons and protons is not equal, an ion with two or more atoms is formed.
- 16. Protons If the atom has more protons than electrons it means that the atom will become a positive ion.
- 17. Electrons If the atom has more electrons than protons it means that it is a negative ion.
- 18. Valence electrons The valence electrons are the electrons in the outermost layer of the atom. They determine the element´s behavior. They are either shared or exchanged.
- 20. Valence electrons Metals usually loose their valence electrons and nonmetals usually gain them in ionic bonds.
- 21. Periodic Table The periodic table has groups and periods.
- 22. Periods There are 7 periods and they run horizontally.
- 23. Groups There are 8 groups (not counting the middle section that has weird-acting metals) and they are vertical. The group number tells you the number of valence electrons.
- 24. Reactivity