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Definition
| potential energy between positive and negative |
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| related to the distance between atoms in a sample of the element |
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| the trend in size changes slightly since electron/electron repulsions counteract the decrease in size as we go across a period |
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| The energy required to remove an electron from an atom in the gas phase |
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| As atomic radius decreases, the ionization energy _____ |
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| The energy change for a process in which an electron is acquired by the atom in the gas phase or “how bad an atom wants an electron.” |
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| Ions that have the same number of electrons (but different number of protons). N-3, O-2, F-, Na+,and Mg+2 |
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| When a chemical reaction occurs between two atoms, their valence electrons are reorganized so that a net attractive force occurs between atoms. |
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| forms when one of more valence electrons is transferred from one atom to another. Produces a positive and negative ion. The “bond” is the attraction between the ions |
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| the sharing of valence electrons between atoms. |
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| Metal with nonmetal bonding – |
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| electron transfer and ionic bonding |
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| occurs most commonly between non mental atoms |
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| Metal with metal bonding – |
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| electron pooling and metallic bonding |
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| metal atoms sharing valence electrons but not by covalent bonding |
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| when atoms bind, they lose, gain, or share electrons to attain a filled outer level of eight electrons or two for H and Li |
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Definition
| the enthalpy change that occurs when 1 mol of ionic solid separates into gaseous ions |
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Term
| Ionic solids exist only because |
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Definition
| the lattice energy exceeds the energy required for the electron transfer |
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Term
| Formation of a covalent bond always results in |
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Definition
| a greater electron density between the nuclei |
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| the number of electron pairs being shared by a given pair of atoms |
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Definition
| the most common band and consists of one bonding pair of electrons |
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Definition
| consists of two bonding pairs of electrons, four electrons shared between two atoms so the bond order is 2 |
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| the energy needed to overcome this attraction and is defined as the standard enthalpy change for breaking the bond in 1 mol of gaseous molecules |
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Definition
| the distance between the nuclei of the two bonded atoms |
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| Bond order to directly related to _____and inversely related to ______ |
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Definition
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| Most covalent substances have low electrical conductivity because |
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Definition
| their electrons are localized and ions are absent |
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Term
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Definition
| the relative ability of a bonded atom to attract shared electrons |
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| An important use for electronegativity is |
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Definition
| determining an atom’s oxidation number |
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Term
| When atoms of different electro negativities form a bond, the bonding pair is shared ____ |
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Definition
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Definition
| unequal distribution of electron density |
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Term
| Electronegativity difference - |
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Definition
| the difference between the electronegativity values of the bonded atoms |
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Term
| Electronegativity difference is directly related to a bond’s _____ |
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Definition
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Term
| As the ∆EN decreases, the bond becomes more ____ |
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Definition
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Term
| Bond Dissociation Enthalpy: |
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Definition
| the enthalpy change for breaking a bond in a molecule with the reactants and products in the gas phase |
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Definition
| When the bond between two atoms has a positive and negative end or pole. |
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| Hydrogen atoms from ____ bonds |
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Definition
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| Carbon atoms from _____ bonds |
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Definition
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| Nitrogen atoms form _____ bonds |
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Definition
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| Oxygen atoms form ______ bonds |
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Definition
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| Fluorine is always a ______ |
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Definition
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Definition
| have the same relative placement of atoms but different locations of bonding and lone pairs |
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Definition
| average of the resonance forms |
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| Partial bonding in resonance hybrid, often leads to ______ |
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Definition
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Term
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Definition
| change an atom would have if the bonding electrons were shared equally |
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Definition
| have fewer than eight electrons around the central nucleus |
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Definition
| species that contain a lone (unpaired) electron, which makes them paramagnetic and extremely reactive |
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Term
| Expanded valence shells occur only with _______ because they have d orbital available |
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Definition
| nonmetals form period 3 or higher |
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Term
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Definition
| to minimize repulsions, each group of valence electrons around a central atom is located as far as possible from the others |
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Definition
| three dimensional arrangement of nuclei joined by the bonding groups |
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Term
| The electron group arrangement is defined by |
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Definition
| the bonding and nonbonding electron group |
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Term
| The Molecular shape is defined by |
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Definition
| the relative positions of the nuclei, which are connected by the bonding groups only |
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Definition
| angle formed by the nuclei of the two surrounding atoms with the nucleus of the central atom at the vortex |
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| Lewis electron dot symbols: developed by |
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Definition
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Definition
| The e- involved in the covalent bond. |
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Definition
| The e- not involved in bonding also called nonbonding e-. |
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Term
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Definition
| The tendency of molecules and polyatomic ions to have structures in which eight e- surround each atom |
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Term
| Valence shell electron-pair repulsion is a method for |
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Definition
| predicting the shapes of covalent molecules and ions. |
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Term
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Definition
| the geometry taken up by ALL the valence e- pairs around a central atom |
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Term
| Molecular geometry describes |
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Definition
| the arrangement in space of the central atom and the atoms directly attached to it. |
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Term
| Valence Bond Theory created by |
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Definition
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Term
| Bonding between the two atoms occurs when |
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Definition
| the e- clouds on the two atoms interpenetrate or overlap |
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Term
| Orbital overlap increases the probability of |
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Definition
| finding bonding e- in this region of space. |
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Term
| The idea that bonds are formed by overlap of atomic orbitals is the basis for |
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Definition
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| The covalent bond that arises from the overlap of the two s orbitals (1 from each H) is called |
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Definition
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Term
| Liquids and solids resist |
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Definition
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Term
| Dipole-Dipole Attraction: |
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Definition
| when one polar molecule encounters another, the positive end of one is attracted to the negative of the other, and via versa. |
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Term
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Definition
| The strong attraction between an electronegative atom with a lone pair and the hydrogen atom of the N--H, O--H, or F--H bond. |
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Term
| Dipole/Induced Dipole Forces: |
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Definition
| polar molecules can induce a dipole in a molecules that do not have a permanent dipole. |
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Term
| As the water molecule approaches the O2 molecule a dipole is induced, this is referred to as _____ |
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Definition
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Term
| The degree to which the e- cloud distorts is called ______ |
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Definition
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Term
| The larger the molar mass the greater the _____ |
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Definition
| polarizability of the molecule. |
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Term
| Dipole/Induced Dipole Forces are weaker than _____ |
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Definition
| electrostatic or dipole/dipole interactions. |
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Term
| Induced Dipole/Induced Dipole Forces are often referred to as _______ |
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Definition
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Term
| London forces arise between |
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Definition
| all molecules both polar and non-polar |
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Term
| London dispersion forces are the only intermolecular forces that |
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Definition
| allow non-polar molecules to interact |
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Term
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Definition
| or evaporation is the process in which a substance in the liquid phase becomes a gas |
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Term
| The standard molar enthalpy of vaporization, ΔvapHo (kJ/mol): |
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Definition
| the energy required to vaporize a sample. |
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Term
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Definition
| when a molecule loses efficient energy to reenter the liquid phase. (exothermic) |
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Term
| Equilibrium Vapor Pressure: |
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Definition
| the pressure exerted by the vapor in equilibrium with the liquid phase. |
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Term
| The tendency of its molecules to escape from the liquid phase and enter the vapor phase, referred to as _______ |
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Definition
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Term
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Definition
| when a specific temp and pressure are reached, the interface between the liquid and the vapor disappears. |
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Term
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Definition
| the temperature at which this phenomenon is observed, and the corresponding pressure, critical pressure |
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Definition
| the resistance of liquids to flow |
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Term
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Definition
| the energy required to break through the surface or to disrupt a liquid drop and spread the material out as a film. |
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