What type of molecules have what intermolecular forces holding them together?
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All molecules have intermolecular forces holding them together.  That is how we have things that are large enough for us to see.  Salt is held together by ionic forces.  Water by hydrogen bonds.  Acetone and ethyl acetate (found in nail polish removers) by dipole-dipole interactions.  Oil by van der Waals or London or dispersion forces (all the same thing).
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Determining structure of molecules.\nIonic structures- The Alkali metal halides are ionic compounds e.g NaCl. Na has a positive charge whereas Cl has a negative charge.\n\nMolecular solids- are held by weak bonds called Van Der waals forces. \n\nMacromolecular structures or giant molecular- have covalent bonds between atoms, these bind all the atoms into a giant molecule e.g Diamond
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Molecules always refer to atoms that have covalent bonds (like a water molecule). Stuff with ionic bonds are just ionic compounds.\n\nMore info: http://misterguch.brinkster.net/covalentcompounds.html
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Group of atoms form a molecule.\n\nA molecule can be made of two or more atoms. This atoms can be of the same type:\n\nCl2, H2, O2...\nO2= an oxygen molecule. It is made of two equal oxygen atoms\n\nOr of different types:\n\nCH4, HCl, NH3...\nCH4 = a methane molecule. It is made of 1 atom of Carbon and 4 equal atoms of hydrogen
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All atoms have intermolecular forces that keep them together as solids or liquids. Adding energy will overcome these forces and cause them to change phase from solid->liquid->gas (with a few that jump straight from solid to gas).\n\nEnergy has to be added to cause this phase change. Going in the opposite direction requires withdrawing energy.\n\nThe types of forces or bonds (not chemical bonds) absorb energy when broken, give up energy when formed. It implies that the solids are in a lower energy state than liquids, and liquids lower than gases.\n\nThis said, when water turns in ice, heat energy is being withdrawn, and the molecules are getting into a more stable and fixed configuration with respect to each other. Because of the polar nature of water, it forms hydrogen bonds between molecules. These type of bonding means when water turns into ice, it positions the molecules into very specific configurations, to maintain the lowest energy state it can get to. Hence the formation of ice crystals.
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Solids, whether pure elements or in general, are crystals made up of ions or molecules, or in rare cases like diamond a single compound of covalent bonds. The thermal stability of a crystal depends on the electrostatic (electrical charge, dipol or quadrupol) property of the constituents and their orientation, as well as their ability to retain constituents placed on the surface to the liquid. Electrostatic forces depend on the charge (or partial charge in case of dipols) and the inverse squared distance of the charges. Quadrupol forces aka Van der Waals forces depend on the inverse sixth potency of the charge.\n\nUsually crystals made up of molecules break up into single molecules when melting. In the liquid these molecules still interact with each other, until at boiling point these interactions aren't strong enough to retain the molecules in the liquid. Crystals made up of ions create ionic melts held together by electrostatic attraction. This isn't found for pure elements, though. Metals are similar in the liquid and solid state, with ionized atoms surrounded by a dislocated electron cloud. Covalently bonded crystals don't melt, but may transform into different compounds.\n\nNote that most elements have several different solid states.\n\nElemental carbon can be found as monomer or low-count polymer fragments in the gaseous phase, no liquid phase (except Buckminster Fullerenes) that I know of and several very different solid phases: graphite (thermodynamically most stable form), diamond, and Buckminster Fullerenes and variations thereof which don't really behave like a solid.\n\nSeveral gaseous elements have no known solids at normal pressure. Iodine has no liquid phase at normal pressure.\n\n\nIn a very general sense, the stronger the attractive forces between the elemental constituents, the more stable the solid/liquid phase. Covalently bonded elements tend to have higher melting points than metals, which in turn tend to have higher melting points than elements occurring in distinct molecules. Quite often the solid and even liquid phases include a change of atomic structure and nature of the bonds. Even in the gaseous phase, sometimes pairing of neutrally charged molecules may occur.
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Intra>>>>>>Forces among atoms of the molecule.\nInter>>>>>>Forces between a molecule and its surrounding molecules.
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TCATTG\n\nT molecules connect with A molecules\nC molecules connect with G molecules
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There are fundamentally many ways to answer this question; and I will address three.\n\nIn nuclear chemistry, there are four fundamental interactions of matter that can be termed energy:\n\n1. Strong interaction, or strong force. This is the force which holds together quarks and other subnuclear particles into discreet protons, neutrons, and electrons. This is the energy that is released in a nuclear reaction.\n\n2. Weak interaction, or weak force. This is the force which holds protons and neutrons together in the nucleus of an atom. This is the energy that is released in radioactive decay.\n\n3. Electromagnetism. This is the attractive or repulsive force caused by the positive or negative charge of atomic particles and the electromagnetic field of photons. This force is the most wide in function, and is present in practically every conventional phenomenon. The electromagnetic force is responsible for electron orbitals, for chemical bonds and reactions, for electromagnetic radiation, and fundamentally for traditional force.\n\n4. Gravity. This is the tendency of objects with mass to accelerate toward each other. This is the weakest force, but can act over an almost unlimited distance.\n\nOR ....\n\nIn classic chemistry, a molecule can have three kinds of energy:\n\n1. Transitional energy, or the energy relative to motion.\n\n2. Chemical energy, or the energy inherent to electrochemical bonds.\n\n3. Vibrational energy, or energy relative to the vibration or oscillation of individual molecules.\n\nOR ...\n\nIn physics, we categorize all energy in the universe into two sets:\n\n1. Potential energy. This is the energy inherent in position or interaction with another body.\n\n2. Kinetic energy. This is the energy a mass possesses relative to its motion, whether it be classic velocity or vibration. This is sometimes termed work, though this is technically incorrect; both kinetic and potential energy are work, in different forms.\n\nAnd there you have it.
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Hydrogen bonding of Water molecules: Due to the polar covalent bonds that hold a water molecule together, Hydrogen bonds form where the negative Oxygens and the positive Hydrogens are located.\nThe results of these bonds are as follows:\n \n1. Cohesion: is the sticking together of similar molecules. Water is very cohesive. This allows water to be pulled along a pathway with relative ease.\n \n2. Surface Tension: cohesion allows water to pull together and form droplets or form an interface between it and other surfaces. The measure of how hard it is to break this interface is its surface tension.\nWater allows materials to rest upon it if the surface tension is not broken. Pollen, dust, water insects, and other biological materials are able to remain on the surface of the water because of this tension.\n3. Adhesion: The sticking of one substance to another. Water is a good adhesive. It will cling on to many objects and act as a glue. Capillary Action is an example of cohesion and adhesion working together to move water up a thin tube.\n\n4. Imbibition: The process of soaking into a hydrophilic substance. Water being taken into a sponge, into a seed, into paper towels.\n\n \n5. High Specific Heat: Specific heat of a substance is the heat needed (gained or lost) to change the temperature of 1g. of a substance 1degree Celsius. Heat is the total quantity of kinetic energy due to molecular motion. Temperature measures the intensity of the average kinetic energy of the molecules.Heat and temperature are not the same thing. A Kilocalorie or large C equals 1,000 small calories.It takes 1,000 calories to raise 1,000g. of water 1 degree C. Nutritional Packaging has the calorie measurements in Kilocalories. One gram of Protein = 3 calories. This means 3,000 small calories or 3 Kilocalories.\nThis high specific heat allows water to act as a heat sink. Water will retain its temperature after absorbing large amounts of heat, and retain its temperature after losing equally large amounts of heat. The reason for this is that Hydrogen bonds must absorb heat to break. They must release heat when they form.The Ocean acts as a tremendous heat sink to moderate the earth's temperature.\n \n6. High Heat of Vaporization: Water must absorb a certain amount of additional heat to change from a liquid into a gas. This extra heat is called heat of vaporization. In humans, this value is 576 cal/g. This results in evaporative cooling of the surface. Alcohol has a value of 237cal/g. and chloroform 59cal/g.\nAs one can see water removes much more heat from a surface upon evaporation than does either alcohol or chloroform.\n \n7. Freezing and Expansion of Water: Water is most dense at 4 degrees C. At ) degrees C. it is 10% less dense. Ice floats because maximum Hydrogen bonding occurs at 0 degrees C.\n \n8. Versatile Solvent: Water is a major solvent in nature. When water and another substance is mixed the resulting solution is called an aqueous solution. Any solution contains the following parts:\nSolute( what's being dissolved) + Solvent ( what is doing the dissolving) = Solution.\nSolute Concentration: The concentration of the dissolved materials in relation to the solvent. This is always measured in moles. A mole is the amount of a substance whose mass is in grams is\nnumerically equivalent to the molecular weight in daltons. One must first find the atomic weights of the substance involved and add them together for the representative molecule and change the value to grams.\nMolarity occurs when the mole (gram atomic weight of the substance) is placed in a container and dissolved in one Liter of water.
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the simplistic answer involves the electrons, protons and neutrons. the more complex answer contains up quarks, down quarks- which are the building blocks of protons and neutrons. \nThen if we think about it we have also got anti-matter, which is involved in bonding and so forth, and so must be around somewhere. positrons, anti-bonding orbitals, etc.
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Chemical bonds form when electrons are shared, like in covalent bonds.  The atoms in the bond share a certain number of electrons between them usually so they both have a complete octet of electrons.  Another type of bond is ionic.  This is when one atom completely pulls off an electron from the other atom.  This results in a negative charge on the taker and a positive charge on the giver.  The bond is formed by the electromagnetic force acting between these two dissimilar charges.
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Covalent bonding is a description of chemical bonding that is characterized by the sharing of one or more electrons between two atoms. In general bonds are defined by a mutual attraction that holds the resultant molecule together. Often bonding occurs in such a way that the the outer electron shells of the participating atoms become filled. In contrast to electrostatic interactions labeled as "ionic bonds," the strength of covalent bond depends on the angular relation between atoms in polyatomic atoms. Covalent bonding is most important between atoms with similar electronegativities. Covalent bonding is often delocalized.
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The simple answer is probably: covalent bond\n\nI quote: "Covalent bonding is an intramolecular form of chemical bonding characterized by the sharing of one or more pairs of electrons between two species, producing a mutual attraction that holds the resultant molecule together. Atoms tend to share electrons in such a way that their outer electron shells are filled. Such bonds are always stronger than the intermolecular hydrogen bond and similar in strength to or stronger than the ionic bond."
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Fluctuating dipole bond: Weak electric dipole bonding can take place among atoms due to an instantaneous asymmetrical distribution of electron densities around their nuclei. This type of bonding is termed fluctuation since the electron\ndensity is continuously changing.\nPermanent dipole bonds: Weak intermolecular bonds are formed between molecules which possess permanent dipoles. A dipole exists in a molecule if there is asymmetry in its electron density distribution.
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Why do atoms not fly apart? After all, the nucleus is a bunch of positive charges all very close together. \n\nAnswer: the strong force holds the nucleus together.
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Molecules exist in different shapes. Many of the physical & chemical prpoerties of molecules arise due to the different shapes.\n\nSome of the common geometrical shapes are trigonal, planar, tetra hedral etc.The VSEPR theory provides a simple treatment for predicting the shapes of polyatomic molecules. The theory was originally proposed by Sigdwick and Powell in 1940. \n\nIn case of molecules with central atom having one or more lone pairs VSEPR treatment is as follows: In these type of molecules, both lone and bonded pairs of electrons are present. The lone pairs are localised on the central atom, & bonded pairs are shared between the two atoms. Consequently, the lone pair of electrons occupy more space as compared to the bonding pair. This causes great repulsion between lone pair of electrons.\n\nThese repulsion effectscause deviations in the predicted bond angles in molecules. \n\nThe descending order of repulsion interaction is lp - lp > lp - bp > bp - bp\n\nlp - lone pair\nbp - bonded pair