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| The way a substance reacts when it comes into contact with another substance or a form of energy. Reactivity depends on the electron configuration of the element. |
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| Nobel gases are the least reactive elements because they have a full octet (8 v.e.)(expecgt He). |
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| Alkali metals (group 1) and the halogens (group 17). The metals need to loose one electron to achieve octet. The halogens need to gain one electron |
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| An atom that has gained or lost electrons and now have a positive or negative charge. All atoms want 8 electrons in the valance shell. They can achieve this by becoming an ion. Ions and their parent atom have different properties. |
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| An ion with a positive charge. Metals become cations. |
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| An ion with a negative charge. Non metals become ions. |
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| A bond that forms between ions of opposite charges. Ionic compounds are called saits. |
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| Why does a chemical bond form? |
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| A chemical bond forms because the individual atoms are unstable. The individual atoms form a bond to become more stable and as a result, potential energy is lowered. |
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| The energy stored within the bonds between atoms. |
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| Energy changes in bonding and stability: |
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| When two atoms bond the potential energy is lowered and they become more stable. |
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| Intramolecular and intermolecular |
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| True bonds and very strong. Covalent(polar, non polar and coordinate), ionic and metallic. |
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| There are attractions, not true bonds. Dipole, hydrogen bond (dna) van der waals and molecule-ion attraction. |
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| How many intramolecular bonds are there? |
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| 3: ionic, covalent and metalic |
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formed by metal and non-metal atoms
formed by a complete transfer of elements
formed by a polyatomic ion and anything that will react with it
electronegativity difference is >1.7 exception: NATL (electronegativity 1.2) metal hdrides |
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form as a result of sharing electrons
only form between non-metals
the difference ion electronegativity is less then 1.7
#3 is only useful for two elements |
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| Non polar covalent bonds: |
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forms as a result of equal sharing of electrons
forms between two atoms that are the same
electronegativity difference is equal to zero
Homonuclear (elemental) diatomics- HOFBRINCL
the charge distribution in all of these atoms is symmetrical |
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formed between 2 different non metals
electrons are shared equally
diffrent electronegativies greater then zero less then 1.7
The electrons are still shared however the atom with the greater elctronegativity will attract the electron with greater force. This will result in a slight positive and negative charge to a polar covalent. |
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| coordinate covalent bonds |
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both electrons to be shared come from one atom
the other atom doesn't have electrons
substances that have an extra pair of electrons can form a coordinate covalent bond. |
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formed by two of the same or different metals
Examples: Na (s) Fe (s) |
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| What are lewis electron dot structures? |
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| a modeling technique that shows how electrons are shared or transferred during bond formation. They consist of the chemical symbol surrounded by the VE |
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| What are lewis diagrams of compounds? |
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Lewis dot diagrams put together so that each atom has or shares 8 electrons (i.e. has its octet)
H is the expection to the octet bond.
Covalent Non Polar |
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| What do we mean by a molecule having symmetry or equal distribution of charges? |
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Polar Molecules: unequal distribution of charges, asymmetrical molecule, made of any polar bond
Non Polar Molecules: equal distribution of charges, symmetrical molecule, made up of non polar and polar bonds |
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| What doe we mean by "like dissolve like"? |
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Polar molecules attract polar molecules (and ions). Non polar molucules attract non polar molecules. Adhesion: attraction between 2 separate molecules of different types
cohesion: internal attraction of the atoms of a molecule of same types or forces. |
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| dipole-dipole attractions |
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| a dipole means a polar molecule. there for a dipole-dipole attraction is an attraction between 2 polar molecules. |
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strongest of all intermolecular attractions.
types of dipole-dipole attraction
forms between a Hydrogen of 1 molecule and either N,O, F of a separate molecule. |
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| Van Der Waals Forces: aka London forces |
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weakest attraction that exists
forms between non polar molecules including noble gasses, large organic molecules and homonuclear diatomic HOFBRINCL |
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| What do we mean by hydrated ions: |
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| NaCl: An ion that is surrounded by water molecules. |
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| Tells you the total number of of atoms of each element in one molecule of a substance |
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| Represents the simplest ratio which the atoms combine to form a compound. The subscripts represents the simplest whole number relationships between the number of atoms of each element in the compound. |
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| Naming Binary and Ionic compounds |
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| (Metals and Non-Metals) These are ionic compounds generally named in the order that the elements appear. The second element ends in -ide |
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| Compounds that are made up of 3 different elements. Many are compounds in which the cation is a metal and the anion is poly-atomic1 |
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| Naming Covalent Compounds |
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| These are generally molecular compounds. The second element end in -ide |
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