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25% of AP Exam questions will cover bonding. I would like for you to explain at least 3 concepts you have learned from this unit. DETAILS!!

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I learned that Hybridization is a process of mixing orbitals in order to make electrons more suitable to form with other orbitals.
2. I also learned about the Vander Wal force. This is attraction and repulsions between atoms, molecules, and surfaces, as well as other intermolecular forces.
3. Lastly I learned that the vsepr theory that predicts the geometry of individual molecules.

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I learned about molecular formula which is the true formula of a compound. This formula shows the exact number of atoms present in a molecule. To calculate, you must find the empirical formula, divide the molar mass by it and multiple the empirical formula by the multiple. I also learned about density which is basically how much stuff is inside an object. To find density, you must divide the mass by the volume. Lastly, i learned about moles, which is a unit of measurement. you use moles to convert to grams and vice versa. one mole equals 6.02x10^23. To calculate, add the masses. To convert moles to grams, you must multiply the number of moles by the mass. if you wanted to convert the other way, you would divide.

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1. hybridization-The manipulation of and or interference to orbitals in order to make electrons more suitable for elements in order to bond.

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1. hybridization-The manipulation of and or interference to orbitals in order to make electrons more suitable for elements in order to bond.

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2. Molecular and electron Geometry- The different and angles and shapes of compounds and molecules within a chemical reaction and or bond. there are all sorts of different shapes and angles like tetrahedral or  trigonal pyramid and angles like 120 for the s2p orbital.
3. The concept of pairing is very interesting as well. when chemical bonds are being put into place the electrons particularly the valence electrons are vital to the chemical bond. Just depending on the bond type like covalent or ionic there can be electrons shared or take/given away.

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One concept I learned about this unit was hybridization. This is the process of mixing orbitals to form new orbitals, hence the term hybridization. Another concept I learned in this unit was the VSPER theory. The VSPER theory deals with the repulsion of valence electrons and determining the shape of the molecules.  I also learned about the different types of intermolecular and intramolecular forces such as hydrogen bonding, dipole-dipole, London dispersion, metallic bonding, polar covalent bonding, and non polar covalent bonding.

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I have learned about sigma bonds. I've learned that they are the strongest covalent bonds. I've also learned about bond hybridization and how it is basically atomic orbitals fuse to form hybridized orbitals. And last I learned VSEPR which is valence shell electron pair repulsion theory. Which is a model that helps predict geometry of a certain number of molecules surrounding their central atoms.

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Has to do with electrons and bonding and like ionic and covalent bonding. together and the electrons gaining and loosing and sharing and the stuff with the bond angles like sp180,sp2-120,sp3-109.5 and how hybridization can affect it. hybridization that's combining and using different orbitals to make bonds. Then u have the vsepr theory where you predict the geometry of individual molecules by the number of electrons paired around the central atom.

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Has to do with electrons and bonding and like ionic and covalent bonding. together and the electrons gaining and loosing and sharing and the stuff with the bond angles like sp180,sp2-120,sp3-109.5 and how hybridization can affect it. hybridization that's combining and using different orbitals to make bonds. Then u have the vsepr theory where you predict the geometry of individual molecules by the number of electrons paired around the central atom.

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The VSEPR theory elaborates on the entire formation of molecular bonding. In which, the formation of bond types, structures, angles, and shapes are examples of this ability to elaborate. These are leading characteristics that have made VSEPR true causing bonding to have a broader understanding. The VSEPR theory includes the Hybridization from the combination of s and p orbitals. With, the introduction of sigma and pi bonds these pertains to ability to understand molecular structure.     Not only VSEPR was about of this unit you must provide Intermolecular and Intramolecular Forces that has to do with the strength/length of the differ bond types. bond 

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The VSEPR theory elaborates on the entire formation of molecular bonding. In which, the formation of bond types, structures, angles, and shapes are examples of this ability to elaborate. These are leading characteristics that have made VSEPR true causing bonding to have a broader understanding. The VSEPR theory includes the Hybridization from the combination of s and p orbitals. With, the introduction of sigma and pi bonds these pertains to ability to understand molecular structure.     Not only VSEPR was about of this unit you must provide Intermolecular and Intramolecular Forces that has to do with the strength/length of the differ bond types. bond 

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Molecular Geometry - The shape a molecule takes based off of the amount of atoms and lone pairs it contains.
Bond Angles - As more lone pairs or atoms are added to the central atom of a molecule, the angles between the bonds are decreased.
Hybridization - Energy levels will merge to create a more stable field for electrons to stabilize a molecule

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I´ve learned that as the number of a bond atoms increase the more the atoms are packed together. I learned the difference between bonding domains and non bonding atoms and what happens to a bond angle when you remove an electron domain. I have also learned that covalent bonds tend to depend on the overlap between the valence orbitals of the bonded atoms.

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I´ve learned that as the number of a bond atoms increase the more the atoms are packed together. I learned the difference between bonding domains and non bonding atoms and what happens to a bond angle when you remove an electron domain. I have also learned that covalent bonds tend to depend on the overlap between the valence orbitals of the bonded atoms.

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What I have learned this unit and remember is hybridization,molecular shapes and vsepr theory. Hybridization deals with combining old and new orbitals and making them one bond(sp orbitals). Molecular shapes deals with tetrahedral, linear, trigonal planar and bypyrim etc. Lastly, vsepr theory deals with the pairing of valence electron shell's and determining the molecular geometry or shape.

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I've learned that that the VSEPR Theory is used to predict the structure of electrons. I've also learned that dipole-dipole forces are the attraction of a positive end and negative end of a molecule and that London Dispersion Forces is the attraction between induced dipoles and temporary dipoles.

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I have learned the difference between covalent bonding and ionic bonding and how you can tell the difference between their characteristics. 1. Ionic bonding is between two ions that form through one or more electrons. The properties is that it can crystalizes it has a high and low boiling point. 2.Covalent bonding is when two atoms are haring an electron pair between two atoms. Its properties is they have low boiling and melting point. they are strong bonds. Then something else i learn that the 3. sp3 hybrid has a 109.5 angle . sp2 hybrid has 120 angle and sp has a 180 angle. I also learned about the Vsepr theory is used to tell the individual molecule from the number of electron pairs.

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1. I have learned about hybridization which is when you mix orbitals which then forms into new orbitals.
2. I learned about London Dispersion forces and how it is an attraction force between polar molecules. Another name for it is vandar wal force. London dispersion forces are weak.
3. I learned about dipole forces and that they are created through a positive and negative poles. A dipole force is a polar molecule that has partially positive and negative poles. Dipole forces only exist through polar compounds and not nonpolar compounds.

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I learned about ionic bonding and that that ionic bonds are always between a metal and a nonmetal. They are also between a cation and anion.

I learned about the octet rule, which is that when some atoms compounds they get the same electron configuration as a noble gas, which means they have 8 valence electrons.

I learned the VSEPR theory, which shows that as new atoms or lone pairs are added to a compunds, the existing atoms or lone pairs repel against the new ones in order to keep them equally spaced apart.

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I learned that when you add a lone pair to the bonds it makes them bend. There are many different shapes and bond angles.

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I learned that when you add a lone pair to the bonds it makes them bend. There are many different shapes and bond angles.

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Ionization
In this period of learning i learned that the element Ca has more ionization than L. This is because it increases from left to right and increase from top to bottom.
Dipole- dipole forces
I learned that a dipole dipole force is made by a positive end of one dipole and a negative end of another dipole.

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In this unit I have learned about the characteristics of ionic, covalent and metallic bonding. Metallic bond involves two metals and are great conductors of electricity and are shiny. Covalent bonds are between 2 nonmetals and they are low conductors of heat and electricity and most are gases. Ionic bonds are between a nonmetal and a metal, they are good conductors of heat and electricty and are electrostatic. I learned of the different intermolecular forces and their bonds. London dispersion forces are the weakest forces because they include a temporary dipole and can occur between any two molecules even polar. Hydrogen bonding is the strongest bond and it has to include a Hydrogen item, which is what makes them stronger when they bond to N, O, or F. The last bond is dipole-dipole which is two polar molecules bonded by the negative and positive ends. It falls between the two previously stated. The last concept I learned about was the VSEPR theory which explains the shape of a molecule based on the way the electrons repel. The electron geometry involves lone pairs while, the molecular geometry involves only bonding electrons. Depending on the number of valence electrons, the bond angle will differ but the SP molecules will always be 180 degrees. A tetrahedral will always be 109.5 and trigonal planars are 120 degrees because they add up to 360 degrees.

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Micah Gosha-I learned about the different types of bonds which are ionic, covalent, hydrogen, and metallic bonds. I remember with an ionic bond they usually have valence electrons that transfer. They transfer onto another which basically goes over the outer electron shell. I also learned that sometimes with chemical bonding they would produce a 3d model of its own bond. With the 3d model it reminds me about the other types of models likes electron geometry. Because it all based off the shapes and the different types of angles within each other.And with the 3d model there are different types such as linear, trigonal planner, tetrahedral.

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Micah Gosha-I learned about the different types of bonds which are ionic, covalent, hydrogen, and metallic bonds. I remember with an ionic bond they usually have valence electrons that transfer. They transfer onto another which basically goes over the outer electron shell. I also learned that sometimes with chemical bonding they would produce a 3d model of its own bond. With the 3d model it reminds me about the other types of models likes electron geometry. Because it all based off the shapes and the different types of angles within each other.And with the 3d model there are different types such as linear, trigonal planner, tetrahedral.

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I learned that hybridization is when different atomic orbitals combine to form one.
I also learned that each atom has a specific bond angle. The atoms repel each other and try to stay as far away from each other as possible. Each atom are place the same distance from each other. The bond angle the molecule is the same all the way around.
I also learned that each molecule has a specified shape. The shapes vary because of the number of atoms and their bond angles.

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One concept I have learned about is Intermolecular forces. Intermolecular forces determine the physical properties of substances. Dipole–dipole interactions, London dispersion forces, and hydrogen bonds are the three types of intermolecular forces. Dipole-dipole interactions are the strongest intermolecular force of attraction.
Another concept is Ionization energy. The second ionization energy is greater than the first because it’s more difficult to remove an electron from a cation. K has the lowest ionization energy. When a group 1 element reacts it

loses one electron. The third concept we talked about is Quantum Numbers. Principal Quantum Number,  Angular Momentum Quantum Number, Spin Quantum Number, and Magnetic Quantum Number are types of Quantum numbers. Quantum numbers specify the arrangements of electrons in orbitals.

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The first thing I learned from this unit was the intermolecular forces. This was the London Dispersion Forces, Hydrogen Bonds, and Dipole-Dipole bonds. The strongest one was hydrogen bonds and the weakest was London Dispersion forces. Another concept I learned was the polarity of covalent bonds. I learned how nonpolar covalent bonds have smaller differences in electronegativities than polar bonds. The last concept I learned was hybridization of the S and P orbital. This is determined by counting the number of atoms and lone pairs connected to it.