Chemistry - Flash Card Set 2

Ch. 5 Ch. 9 Ch. 10

what is electromagnetic radiation (EM)?

a form of energy (also known as light) and is described in waves

what is wavelength (λ)?

the distance between the peaks of each wave

what is a photon?

a particle of light

what is the formula between wavelength (λ), frequency (v), and speed of light (c)?

c = λv ; v = c/λ ; λ = c/v

how are wavelength and frequency related?

inversely related ; shorter wavelength, higher frequency and longer wavelength, lower frequency

what is the electromagnetic spectrum?

the variety of light and which kind we can see based on their wavelengths

what colors are associated with wavelength?

reds = long wavelength/low frequency ; blues = short wavelength/higher frequency

what is the formula to calculate the energy of a photon?

E = hv ; E is energy (in J), h is Planck’s Constant (6.626 × 10⁻³⁴Js), v is the frequency (in s⁻¹)

the farther the energy level is from the nucleus…

the higher the energy of the electrons

what is “ground state?”

when electrons fill up the lower energy levels first and as new ones are added, go into higher levels

what is “excited state?”

when electrons get the energy to jump from its current energy level to a higher one

what is absorption?

electron gains potential energy and moves farther from the nucleus

low potential energy → high potential energy

what is emmission?

electron loses potential energy and moves closer to the nucleus

high potential energy → low potential energy

one way an electron can give off energy to return to ground state is…

through the form of light (emission)

what are orbitals?

shapes that describe the regions where an electron is likely to be found; a complete set of orbitals in a given energy level is called a subshell

list the 4 common orbital types and their shapes

1. s orbital - spherical

2. p orbital - dumbell

3. d orbital - clover and donut with lobe above and below

4. f orbital - complex tetrahedral

how many orbitals are there in each energy level and how many electrons can each orbital hold?

1. one s orbital - 2 electrons

2. three p orbitals - 6 electrons

3. five d orbitals - 10 electrons

4. seven f orbitals - 14 electrons

how can you categorize electron configuration on a periodic table?

what is electron quantization?

the orbitals in an atom can only have a specific set of values; an electron requires a particular amount of energy to either give or release in order to move it to a different energy level

what is electron configuration?

when each element has its own unique configuration that describes which subshells have electrons and how many

example: Boron = 1s²2s²2p¹

what are orbital diagrams or the “spinning” property of electrons?

a graphical form of electron configuration, representing the mass and charge of electrons as arrows and which directions they spin (up or down); Hund’s Rule: ground state atoms will fill unoccupied orbitals first

what are the types of periodic trends?

what are valence electrons and how do you find them?

the electrons occupying the outermost energy levels of an atom are called the valence electrons and are responsible for chemical bonding; for elements in group 1A-8A, the number of valence electrons in an atom is simply the group number

simply put, how do you draw Lewis dot strucures?

the chemical symbol in the center, surrounded by as many dots as that atom has valence electrons

what is the Octet Rule?

atoms react in such a way as to give them 8 electrons in their outermost energy level (valence shell); noble gases usually do not react because their shell is already filled with 8

what is the Duet Rule?

hydrogen atoms attempt to pick up another electron to give the same configuration as Helium

what are the types of bonding?

ionic: mutual attraction of oppositely charged ions through the gain or loss of electrons of an atom (metals & nonmetals)

covalent: a pair of electrons shared by two atoms

what is the VSPER theory?

Valence Shell Electron Pair Repulsion: electron pairs move as far away from each other as possible; electrons all have negative charges so they repel one another, implying a specific angle

how do you find the polarity of a bond?

if two atoms which are covalently bonded have substantially different electronegativity values (> 0.4 units) then the bond is polar covalent

what are polar and non-polar covalent bonds?

polar: unequal sharing of electrons

non-polar: equal sharing of electrons

what is a dipole moment?

when electrons are drawn to more electronegative atoms which develop a “partial negative charge” and a “partial positive charge” on opposite sides; only occurs in polar molecules

atomic elements are…

all metals and noble gases

non-metal elements are…

molecular

seven common diatomic molecules

H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

molecular (covalent) compounds are made of…

non-metals

ionic compounds are made of…

metal + non-metal and polyatomic ions

elements are

atomic and molecular

compounds are

molecular and ionic

an ionic compound should have what kind of charge?

no total charge (they neutralize)

in ionic compounds, the cation is always listed

first

what are polyatomic ions?

ions which are derived from two or more atoms; molecules that have collectively gained or lost electrons to become an ion

ions are held together by…

covalent bonds

polyatomic ions can contain both

metals an non-metals

which is the only commom polyatomic cation?

NH₄+

the classifications of compounds include…

binary non-metals (molecular compounds) and ionic compounds

binary non-metals are made of…

non-metal + non-metal

ionic compounds are made of…

cation + anion

how do you name binary nonmetal compounds?

prefix + name of 1st element and prefix + base name of 2nd element + -ide

what are the first 10 prefixes and their numerical values?

1. mono-

2. di-

3. tri-

4. tetra-

5. penta-

6. hexa-

7. hepta-

8. octa-

9. nona-

10. deca-

what should H₂O, NH₃, and PH₃ always be called?

water, ammonia, and phosphine

when do you not use prefixes in naming binary nonmetal compounds?

when hydrogen (H) appears first

what does (g) and (aq) mean?

“gas” and “aqueous" (can dissolve in water)

aqueous (aq) compounds are named as…

acids with -hydro as a prefix and -ic as a suffix

when naming compounds, prefixes are only used for…

binary nonmetals

how do you name individual cations?

the name of the metal + “ion”

how do you name individual anions?

change the ending of the element’s name to “-ide”

how do you name ionic compounds?

the name of the cation + the name of the anion

what are hydrates?

an ionic compound which has a fixed amount of water molecules within its structure

for every one unit of a particular molecule, there is a subsequent amount of water molecules associated with it

what are oxyanions and how do you name them?

an anion containing different numbers of oxygen atoms but have the same charge

“-ite” before “-ate”

less oxygen than “-ite” = “hypo”

more oxygen than “-ate” = “per-”

how do you name oxyanions containing hydrogen?

the H is always listed first and the normal charge of the ion is changed by +1 or even +2

prefix “bi-” or the word “hydrogen” before the name of the anion

what is an oxyacid and how do you name it?

compounds which contain exactly as many H+ ions as are necessary to cancel out the negative charge of an oxyanion

“-ous” before “-ic”

“-ite” before “-ate”

what is the mole (mol) and how much is just one of it?

the mole (mol) is a unit of quantity in chem that is used to count large numbers of submicroscopic pieces of matter (such as atoms)

1 mol = 6.022 × 10²³

how do you find # of atoms? how do you find # of mol?

(mol) x (Avocadro’s number) = atoms

(atoms) / (Avocadro’s number) = mol

what is molar mass?

the mass of 1 mole of atoms in grams

atomic mass (amu) = molar mass (grams)