Intro to General Chemistry
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Which of the following particles form the nucleus of the atom? Select all that apply. a) proton b) neutron c) electron
proton and neutron
What is the approximate mass of a proton? a) 1 amu b) 0 amu
mass of proton = 1 amu
What is the approximate mass of an electron? a) 1 amu b) 0 amu
mass of electron = 0 amu
What is the approximate mass of a neutron? a) 1 amu b) 0 amu
mass of neutron = 1 amu
What is the atomic number and what is the single letter abbreviation for it?
number of protons Z
What is the mass number? What is its single letter abbreviation?
number of protons + neutrons A
What are isotopes?
elements that have the SAME number of PROTONS but DIFFERENT number of NEUTRONS
TRUE or FALSE: Elements of the same period are most likely to react in similar ways.
FALSE –> Elements of the same GROUP are most likely to react in similar ways
What are the 4 quantum numbers and what do they describe?
n = principle quantum number --> energy level and distance from nucleus l = angular momentum quantum number --> orbital shape (s, p, d, f) ml = magnetic quantum number --> orbital orientation (px, py, pz) ms = spin quantum number --> spin of the electron
What are the possible values for each of the quantum numbers?
n = 1, 2, 3, ... l = n-1 ml = -l to +l (e.g. 3 ml values for l = 1) ms = +1/2 (up) or -1/2 (down)
What are the orbital shapes (spdf) for the following l values? What are the n values? l = 0 l = 1 l = 2
l = 0 --> s --> n = 1 l = 1 --> p --> n = 2 l = 2 --> d --> n = 3
What is the Aufbau principle?
electrons occupy lowest energy level first (e.g. 1s before 2s)
What is Hund’s rule?
electrons will fill all subshells SINGLY before pairing up
What is the Pauli Exclusion Principle?
no 2 electrons in an atom can have the same set of quantum numbers
What is the spdf notation for carbon (C)? Provide both full and abbreviated forms.
full –> 1s^2 2s^2 2p^2 abbreviated –> [He] 2s^2 2p^2
TRUE or FALSE: electrons always lose the outer most (highest n) electrons first.
TRUE e.g. Co loses one electron… Co = [Ar] 4s^2 3d^7 –> Co = [Ar] 4s^1 3d^7 [CORRECT] Co = [Ar] 4s^2 3d^7 –> Co = [Ar] 4s^2 3d^6 [WRONG]
TRUE or FALSE: Electrons can move to different energy levels to fill orbitals in such a way that subshells are half-filled or completely filled.
TRUE –> Half-filled or completely filled subshells are more stable.
What does diamagnetic mean in terms of electron configuration?
all electrons are paired up –> magnetic fields cancel (no net magnetic field)
What does paramagnetic mean in terms of electron configuration?
unpaired electrons present –> NET magnetic field
Metals ___a___ electrons and form _____b_____ to obtain noble gas configuration. a) lose/gain b) cation/anion
metals lose electrons –> form cations
Non-metals ___a___ electrons and form _____b_____ to obtain noble gas configuration. a) lose/gain b) cation/anion
non-metals gain electrons –> form anions
An ionic bond forms between a/an _____________ and a/an ______________.
metal and non-metal
A covalent bond forms between a/an _____________ and a/an ______________.
non-metal and non-metal
What is the most electronegative atom on the periodic table?
Fluorine Remember: F O N Cl –> uncle FONCl lol