| A | B |
|---|
| The ability of an atom in a molecule to attract electrons to itself is called what? | Electronegativity |
| _____?____ is a ____?____ term whereas electron affinity deals with isolated atoms in the gas phase. | Electronegativity , bonding |
| The energy change when an electron is added to a substance----deals with isolated atoms in the gaseous phase. | Electron Affinity |
| The sharing of electron pair(s) in a bond between two atoms. | Covalent Bond |
| The complete transfer of electrons from one atom to another to form ions,CHARGED ATOMS. | Ionic Bond |
| The ______?_____ of the oppositely charged ions is the ionic bond. | electrostatic attraction |
| A _________?_________ is an EQUAL SHARING of SHARED ELECTRON PAIR(s) in a bond. | Pure covalent bond |
| A _______?________ is an UNEQUAL sharing of electrons between atoms. | Polar covalent bond |
| Ionic bonds form when there is a _____?___ difference in ______?____ between the two atoms bonding together. | large , electronegativity |
| Ionic bonding usually occurs when a metal with ______?____ electronegativity is bonded to a nonmetal having a _______?______ electronegativity. | small , large |
| A pure covalent bond forms between atoms having ________?______ or _________?________ electronegativities. | identical , nearly identical |
| A polar covalent bond forms when there is an ______?____ electronegativity difference between bonding atoms. | intermediate |
| In general, _______?_____ form together by forming covalent bonds, either pure covalent or polar covalent. | nonmetals |
| Ionic bonds form due to __________ electrostatic attraction between two oppositely charged ions. | strong |
| Covalent bonds form because the ____?___ electrons in the bond are attracted to the two different ______?____. | shared , nuclei |
| The _______?_____ to another ______?___ overrides the added ____?_______- ______?_______ repulsions. | attraction , nuclei ,electron-electron |
| _______?_____ are LARGER than the neutral atom and _____?____ are smaller than the neutral atom. | Anions , Cations |
| For _____?____ , the added electrons _____?_____ the electron-electron repulsions. | anions , increase |
| To counteract the increasing of electron-electron repulsions in anions, the size of the electron cloud ___?___ , placing the electrons _______?_____ from one another. | increases , further apart |
| For ______?____, as ______?___ are removed , there are _____?___ electron-electron repulsions and the electron cloud can be _________?______ the nucleus. | cations , electrons , fewer , pulled closer to |
| Condition of having same number of electrons. | isoelectronic |
| Isoelectrocity has ____?___ variables , the number of ____?___ and the number of electrons determine the _____?___ of an ion. | two , protons , size |
| If the number of electrons remain constant, chemists only have to consider the ______?______ to predict ______?_____ in ionic size. | number of protons , trends |
| The ion with the ______?____ attracts the same number of ______?___ most strongly resulting in a smaller size ion. | most protons , electrons |
| The change in energy that takes place when separated gaseous ions are packed together to form an ionic solid is called what? | Lattice Energy |
| Ionic compounds form due to extremely favorable lattice energy values, what would be considered an extremely favorable lattice energy value(s) such that ionic compounds are favored to form? | Large and Negative |
| There are many processes that occur when forming an ionic compound from the elements in their standard state.Most, if not all, of these processes are unfavorable , that is _____?______.However, the large and exothermic lattice energy value dominates and the ionic compound forms. | endothermic |
| Lattice energy follows what law? | Coulomb's Law |
| In general, ionic compounds want _____?_____ , but only up to the point where _______?_______ are removed or added. | large charges , valence electrons |
| When we go BEYOND the valence shell, the energies become very _______?_____ for ionic formation. | unfavorable |
| When ____?_____ bare converted into products, reactant bonds are broken and _______?_______ are formed. | reactants , product bonds |
| ________?______ give good estimates for gas phase reactions, but give poor estimates when solids or liquids are present because the calculation of these ignore the attractive forces holding solids and liquids together. | bond energies |
| ___?_____ have molecules that are very far apart and they have minimal (actually assumed ZERO) attractive forces. | Gases , minimal |
| For an ______?____ reaction, stronger bonds are formed in the products as compared to the strength of the bonds broken in the reactants so energy is ______?___. | exothermic , released |
| For _______?________ reactions, the product bonds are weaker overall and the energy must be _____?____. | endothermic , absorbed |
| As the number of bonds increase, ________?______ increases and bond length decreases. | bond strength |
| Nonmetals which form covalent bonds have _____?____ electrons in the ____?____ and _____?____ orbitals. | valence , s , p |
| How many TOTAL orbitals are there in the sum of s and p orbitals? | four , thus only room for eight total valence shell electrons (octet rule) |
| What is the element hydrogen's valence shell? | 1s orbital, which can only hold potentially two electrons so this element follows the "duet" rule as opposed to the "octet" rule. |
| Drawing _____?____ structures is mostly trial and error, 1st step being to ___?__ the available valence electrons then attach the bonded atoms with a _______?______, this is called a "_________?_______". | Lewis , sum , single bond , skeletal structure |
| In general, when drawing Lewis structures, the atom listed 1st in compound is called the _______?___ atom while all other atoms listed are attached (or bonded) to this main atom. | central |
| The FINAL step in drawing Lewis Structures is to _____?____ the remaining electrons around the various atoms to satisfy the ______?___ for all atoms (or duet rule for H ). | arrange , octet rule |
| In general , molecules and ions always follow the octet rule unless it is impossible.The three types of exceptions are molecules/ions with _____?_____, molecules/ions with an ___?___ number of electrons, and molecules/ions with ____?____ electrons. | too few electrons , odd , too many |
| Which atoms sometimes will not obey the octet rule because they have fewer than eight electrons around them? | Beryllium (Be) and Boron (B) |
| Always satisfy the octet rule when you can, with the exceptions to the octet rule occuring only when ____?____. | there are no other options, that is , it would be impossible to satisfy |
| What is being ddescribed? Holds groups of atoms together, can be ionic, covalent, or polar covalent. | chemical bonds |
| Ratio of (measured dipole moment of X---Y ) and (calculated dipole moment for X+Y- ) times 100% | percent ionic character of bond X---Y |
| The relative ability of an atom to attract shared electrons. | definition of electronegativity |
| This depends on the electronegativity difference of bonded atoms. | polarity of a bond |
| This determines whether or not a molecule will have a dipole moment. | the Spatial Arrangement of Polar Bonds |
| Has a DIFFERENT(smaller or larger) size than does its parent atom. | ion |
| The change in energy when ions are packed together to form an ionic substance..What is this statement? | definition of Lattice Energy |
| This energy is neccessary to break covalent bonds and will increase as the number of shared pairs increases between atoms, and this can be utilized to estimate the enthalphy change for a chemical reaction. | definition of what bond energy is |
| The atoms of the elements of the ____?___ can exceed the octet rule. | 3rd row of Periodic Table and beyond |
| When there are several nonequivalent Lewis Structures that can be drawn for a molecule, ______?_______ is used to choose the most appropiate structure(s). | formal charge |
| What does the term RESONANCE mean in referencing Lewis Structures? | several equivalent lewis structures can be drawn for a molecule |
| Stable molecules usually contain atoms that have their _____?_____ filled leading to a duet rule for hydrogen, an octet rule for 2nd row elements , although some elements in 3rd or beyond rows can violate the octet rule. | valence orbitals |
| This idea is based on the belief that electron pairs will be arranged around a central atom in a way that minimizes the electron repulsions, and this concept can be used to predict the geometric structure of MOST molecules. | VSEPR model (aka Valence Shell Electron Pair Repulsion model) |
| What are the two typical requirements for a polar molecule? | polar bonds and a structure such that the bond dipoles of the polar bonds do not cancel. |
| Why is carbon dioxide , CO2 , nonpolar? | the individual bond dipoles cancel each other out |
| To predict polarity in Lewis Structures, draw the individual bond dipoles, then sum up the _____?____ of the bond dipoles on each other. If this is to have the bond dipoles cancel each other out, then the molecule is nonpolar.If this is to NOT cancel each other out, then the molecule will have a partial _____?___ end and a partial negative end because this molecule is polar. This is called a DIPOLE MEMENT or a POLAR MOLECULE. | net effect , positive |
| Electronegativities of elements ____?____ from left to right across the Periodic Table and ____?____ from top to bottom. Hydrogen (H) has an electronegativity value between Boron (B) and ___?___ in the 2nd row and identical to phosphorus in the 3rd row. | increases , decreases , carbon(C) |
| Generally, if you know where _____?_____ fits into the electronegativity trend, ESPECIALLY for rows 2 and 3, then you can predict bond dipole directions for nonmetals bonded to this element. | hydrogen |
| Hydrogen(H) has an electronegativity value between Arsenic (As) and selenium (Se) in row 4 and identical to ______?____ in row 5. | tellurium (Te) |
