Chemistry Chapter 1: Atomic Structure (2 Stars) Flashcards
Where are protons found?
In the nucleus
What is the fundamental unit of charge?
1.6*10-19C
What is the atomic mass unit of a proton?
1 amu
What does Z represent on an element? What does it represent (# of ______)
atomic number
protons
The sum of the protons and neutrons in the atom’s nucleus is known as ____________.
Mass Number (A)
Can an element have a variable number of protons or neutrons?
Neutrons
How many neutrons does Deutrium have?
(1) has one proton and one neutron and
an atomic mass of 2 amu
How many neutrons does Tritium have?
(2) has one proton and two neutrons and an atomic mass of 3 amu.
The electrostatic force of attraction between the unlike charges of the proton and electron is far lesser or greater than the gravitational force of attraction based on their respective masses.
Greater
The electrons closer to the nucleus are at higher or lower energy levels, while those that are further out have higher or lower energy.
lower energy levels
higher energy.
Valence electrons in ______ bonds allows elements to fill their highest energy level to increase stability.
covalent bonds
The nucleus contains the protons and _____, while the ______ move around the nucleus
neutrons
electrons
The _____ number is the number of protons in a given element
atomic
The mass number is the sum of an element’s _____ and neutrons
protons
The atomic mass of an atom (in amu) is nearly _____to its mass number,
equal
The mass number or weighted average of these different isotopes is referred to as the atomic weight and is the number reported on the Periodic Table.
weighted average
Avogadro’s number?
6.02 × 10^23
What is Planck’s quantum theory?
Energy is emitted as electromagnetic radiation from matter exists in discrete bundles called quanta.
E = hf
Define each measure
The energy of a quantum,
E = hf
where h is a proportionality constant known as Planck’s constant, equal to 6.626 × 10 J·s, and f
(sometimes designated by the Greek letter nu, ν) is the frequency of the radiation.
E= hc/λ
Define each measure
h is Planck’s constant,
c is the speed of light in a vacuum and
λ is the wavelength of the radiation.
Note this is just a combination of two other equations: E = hf and c = fλ.
Lyman series?
The group of hydrogen emission lines corresponding to transitions from energy levels n ≥ 1 to n = 1
Transition b/t upper levels
The group corresponding to transitions from energy levels (upper levels) n ≥ 3 to n = 2 is known as the _____ series
Balmer series
For electrons to move from a lower energy level to a higher energy level, they must ____ the right amount of energy to do so.
absorb
When electrons move from a higher energy level to a lower energy level, they ____ the same amount of energy in the form of light. (aurora borealis)
emit
What is the equation for moles?
M = mass of sample/molar mass
The ___________ states that it is impossible to know both an electron’s position and its momentum exactly at the same time.
Heisenberg uncertainty principle
Pauli exclusion principle?
No two electrons in a given atom can possess the same set of four quantum numbers.
The azimuthal quantum number, ___, describes the subshells within a given principal energy level (s, p, d, and f).
l
The _____ quantum number, ml, specifies the particular orbital within a subshell where an electron is likely to be found at a given moment in time.
magnetic
The principal quantum number, ___, describes the average energy of a shell
n
The____ quantum number, ms, indicates the spin orientation 1 2 ( ) ± of an electron in an orbital.
spin
Electrons fill the principal energy levels and subshells according to increasing energy, which can be determined by the____rule.
n + l rule.
_______ materials have unpaired electrons that align with magnetic fields, attracting the material to a magnet
Paramagnetic = unpaired electrons
Diamagnetic materials have paired or unpaired electrons, which cannot easily be realigned; they are repelled by magnets.
Diamagnetic = parried
Di = 2
The electron configuration uses ___________ (combining the n and l values as a number and letter, respectively) to designate the location of electrons
spectroscopic notation
