Exam Pt. 1 Flashcards
(24 cards)
What is the octet rule?
Elements are more stable with a full valence shell (8 electrons).
What is a cation?
loss of e- over all charge positive
what is an anion?
gain of e- overall charge negative
what is isoelectronic?
ions containing the same # of electrons but protons and neutrons are different.
what is an isotope?
a version of an element with the same number of protons but different number of neutrons.
what is a radioisotope?
atoms that contain an unstable nuclei.
what are some properties of Ionic compounds?
Hard and brittle
high melting and boiling points
counduct electricity when dissolved in water.
What elements are diatomic?
HOFBrINCl never a single atom ex. O2
What are ionic compounds?
What are binary molecular compounds?
(metal + non-metal)
(non-metal non-metal) use prefixes
What is an Ionic bond?
e- are transferred from one atom to another atom, forming ions.
What is a covalent bond?
e- are shared between atoms.
What is a polar covalent bond?
e- are not shared equally between atoms
What is a nonpolar covalent bond?
e- are shared equally.
what is a dipole?
it is an unequal distribution of e-, resulting in a slightly positive end in polar covalent bonds.
What is Intermolecular forces?
Chemical bond covalent or ionic
what is an intermolecular force?
Not a bond! found between covalent molecules.
What is hydrogen bonding?
not a bond.
highly electronegative elements FON attached to a H-atom.
Strongest.
What is dipole dipole?
formed between polar molecules containing opposite charged dipoles.
What is london dispersion?
temporary dipoles
occurs in all types of molecules.
weakest and not that important.
what is the atomic radius and what is its trends?
Distance from the nucleus to the outer most e-.
(across) more protrons= stronger attraction pulling e- closer.
(down) More electron shells added.
what is Ionization energy and its trends?
energy required to remove e-
(across) e- held more tightly due to greater nuclear charge.
(down) e- are further away from the nucleus easy to remove.
what is electronegativity and its trends?
atoms ability to attract shared e- bond
(across) Atoms have more protons and stronger pull on e-.
(down) larger atoms means weaker pull on bonding e-.
what is electron affinity and its trends?
The energy change when an atom gains e-.
(across) More negative. atoms have stronger nuclear attraction, filling their valence shell.
(down) less neg atoms are larger so added e- are farther from the nucleus and feel less attraction.
what is the rectivity on the periodic table?
As you go down the PT the elements become less stable and more reactive.
