Unit 1 Flashcards
(78 cards)
1
Q
What is a Proton
A
-positively charged
- in nucleus
- weighs 1 amu
2
Q
What is a Neutron
A
-negatively charged
- in nucleus
- weighs 1 amu
3
Q
What is an electron
A
-negative
-in cloud
- weighs 0 amu
4
Q
What is an element
A
substance made of one type of molecule
-Pb
-H2
-S8
5
Q
What is a molecule
A
Substance made of more than one atom. Can be the same or different atom
- H2
-CH4
6
Q
What is a compound
A
Substance made of more than one type of molecule
-CH4
-SO4
a compound is always a molecule
7
Q
What is a single atom called?
A
an element
8
Q
What are two of the same atoms called?
A
an element and a molecule
9
Q
What are two different atoms called?
A
a molecule and a compound
10
Q
What is the atomic Theory?
A
- elements are made of atoms and all atoms of an element have the same properties, while different atoms have different properties
- compounds are combinations of different elements but the umber of atoms in a compound is integral and consistent
- atoms can’t be created or destroyed, they just change partners
11
Q
What is atomic number
A
-number of protons
- always constant in an element
- goes above the atomic symbol
12
Q
How is atomic mass labeled?
A
grams per mole
13
Q
What is atomic mass
A
- sum of protons and neutrons
- number of protons = number of electrons unless it is an ion
- goes under the atomic symbol
14
Q
What is molar mass
A
mass of one mole of a substance
15
Q
How can you take the mass of a compound
A
add the masses of each element
15
Q
How can you take the mass of a compound
A
add the masses of each element
16
Q
Which atomic label characterizes an element?
A
atomic number
17
Q
What is an Isotope?
A
- atoms with same atomic number but different mass numbers
- same number of protons but different number of neutrons
18
Q
When is an atom neutral
A
when it has the same number of protons and electrons
19
Q
What is an ion
A
when electrons are added or subtracted from an element
20
Q
What is a cation
A
-electrons are subtracted
- element becomes positive
21
Q
What is an anion
A
-electrons added
-element becomes negative
22
Q
What is the periodic table organized by
A
- organized by Mendeleev based on atomic number and reactivity
- predicted missing elements
-columns/ groups
-periods/ rows
23
Q
How can you tell atomic characteristics
A
- by groups/ columns/ family
- has similar characteristics and reactivities
24
Which way does a group/family go?
vertically
25
Which way does a period go?
horizontally
26
Characteristics of non-metals
- right side of periodic table
-gains electrons easily
27
Characteristics of metals
-left side of periodic table
-loses electrons easily
28
Characteristics of metalloids
-shared characteristics of metals and non-metals
29
Noble gas characteristics
-very stable
- fairly unreactive
-all gasses at room temp
30
Halogen characteristics
-gains one electron very easily to become noble gas
31
Transition metal characteristics
- malleable
-good conductors
- most are solid at room temp
- can lose a varying number of electrons
32
Alkaline earth metal characteristics
- group 2a
-easily looses 2 electrons
33
Alkaline metals characteristics
-group 1a
- very reactive
- reactivity increases as you go down
-malleable, ductile, good conductors
34
lanthanide characteristics
- very reactive
-lose electrons easily
35
actinides characteristics
- radioactive and unstable
-only able to be made in a lab setting
36
what is energy
the ability to do work
37
what is kinetic energy
energy of motion
38
how is kinetic energy measured
by temperature
39
what is potential energy
energy due to position
40
what does potential energy show
how atoms interact or how they are stored
41
What are examples of potential energy
bonds or electrostatic attention
42
What energy state does nature like
low energy state
43
What happens when energy is released
it goes from high to low potential
44
What does Columb's law describe
energy between two particles
45
What are Columb's law rules
1. energy decreases when charges are of opposite signs and increase when they are the same sign
2. is proportional to the charges of the particles
3 is inversely proportional to the distance between them
46
What is Columb's law formula
e= (charge of 1 x charge of 2) / distance between the particles
47
What does a long wavelength mean
- low frequency and low energy
48
What does a short wavelength mean
- high frequency and high energy
49
What is the photoelectric effect
- if a photon doesn't have enough energy to eject an electron it won't if it does it will
-light is a photon (an energy source)
- different wavelengths will have different effects on matter
50
How does light interact
1 photon at a time
51
What does light represent?
electrons going from high energy to low energy
52
How do electrons move energy levels
by absorbing or emitting photons
53
What does emitting a photon mean?
-higher energy level to lower energy level
-overall energy decreases
54
What does absorbing a photon mean?
- lower energy level to higher energy level
-overall energy increases
55
What is Bohr's model?
- electrons orbit the nucleus in quantized radii
-electrons are allowed in state have a certain amount of energy
- the closer to the nucleus the electron is the more stable the electron is
56
What is wave particle duality?
Every particle can be described as a particle or a wave
57
How is light like a wave
c= wavelength x frequency
58
How is light like a particle
e= hv
59
How is an electron like a wave
the quantum theory
60
How is an electron like a particle
- Bohr's theory
-a subatomic particle with a small mass
61
What is the quantum theory
- treats electrons as waves to show their energy and orbitals
- electrons and the orbitals in which they reside are differentiated and described by quantum numbers
- no two electrons can have the same quantum number
62
What is n
- the principal quantum number
- a non-zero positive integer
- describes the distance from orbital to electron
- dictates the size of the orbital
higher n= higher energy
63
what is l
- the number of nodal planes in the orbital
- = n-1
- electrons can't be found here (if l= 1 there is one place and electron can't be found)
64
What are the l values
- 0= s = 2 electrons = 1 orbital
-1 = p = 6 electrons= 3 orbitals
-2 = d= 10 electrons = 5 orbitals
-3 = f- 14 electrons= 7 orbitals
65
what is ml
- determines orientation of the orbital
- goes from -l to 0 to l
66
what is ms
- +/- 1/2
keeps quantum numbers from being the same
67
how can you tell electron energy
n + l
the higher n has more energy
68
what is the Pauli exclusion principle
no two electrons can have all four quantum numbers the same (arrows have to face different ways)
(cannot break this rule)
69
what is the ground state/ Hund's rule
each orbital has an electron before a second electron is added, the number of electrons facing the same way is maximized
(you can break this rule its then just excited)
70
what is paramagnetic
one or more unpaired electrols
71
what is diamagnetic
no unpaired electrons
72
which electrons are better at shielding
core electrons, the closer to the nucleus the better it is at shielding (smaller n + smaller l = better at shielding)
73
what are valence electrons
electrons in an unfilled orbital
74
What is Zeff
- effective nuclear charge
- nuclear charge experienced by valence electrons
75
What is the Zeff formula?
atomic number- number of core electrons
76
what is ionization energy?
- minimum energy input required to remove the highest energy electron present in an element
- the measure of how tightly an electron is bound
- it is easier to remove an electron from an orbital with a higher n value
77
What is electronegativity
- the ability of an atom to attract electrons to itself when it is engaged in bonding to another atom
- higher electronegativity= higher density
- noble gases don't follow electronegativity rules
