Gen Chemistry Flashcards
1
Q
Alpha decay is
A
Two protons and two neutrons (-4 from up and -2 down - atomic number
2
Q
Beta decay is
A
+1 electron
3
Q
Electron capture is
A
-1 electron (beta plus decay)
4
Q
Only … tend to lose or gain as many electrons as needed to achieve a full octet
A
Neutral atoms
5
Q
Definition of effective nuclear charge
A
Measure of the amount of charge from the nucleus of an atom or ion that exerts electrostatic attraction on its valence electrons
6
Q
Formula of Zeff
A
Zeff= Z (total charge= total number of protons) - S (core electrons =10)
7
Q
Electron configuration order
A
1s 2s 2p 3s 3p 4s 3d 4p 5s
8
Q
Types of beta decay
A
B- decay is electron emission, B+ is positron emission and electron capture (decreases atomic number, proton to a neutron) while the mass number is the same
9
Q
Volume formula
A
Mass/volume
10
Q
As temperature decreased the density of the solution … and objects .. while when the t increases..
A
Increases, floats
Density decreases and object sinks
11
Q
1 mole is how many units and g ?
A
6* 10^23 units and mass of the molecule in g
12
Q
Name of the reaction when both the oxidation and reduction occurs to atoms of the same element
A
Disproportionation reaction
13
Q
Slope
A
(y2-y1) / ( x2 -x1)
14
Q
What agent get oxidized and causes reduction in another atom
A
Reducing agent
15
Q
What agent that gets reduced and causes oxidation in another atom?
A
Oxidizing
16
Q
Formal charge formula
A
Valence electrons - no binding electrons- 0.5 bonding electrons
17
Q
Oxidation state formula
A
Group valence - non bonding electrons - assigned bonding electrons ( electrons are given to the most electronegative atom of the bond)
18
Q
Molarity formula
A
Mol / volume
19
Q
Principal quantum number is
A
n shell describes main energy level of the electron
Distance of an orbital from the nucleus
20
Q
Sub shell is
A
Shape of an orbital s, p, d, f and holds 2,6,10,14 electrons
21
Q
Diamagnetic means
A
All electrons are paired and repelled by external magnetic field
22
Q
Paramagnetic means
A
Unpaired electrons that pulled into external magnetic field
23
Q
Gamma emission means
A
Change in energy, mass number and atomic number are not changed
24
Q
As IE increases the Reactivity of atoms …
A
Decreases and vice versa
25
Definition of electronegativity
Tendency of an atom to attract electrons within a bond
26
Definition of electron affinity
Tendency of an atom to accept an additional electron by measuring the energy change when an electron is added
27
Definition of ionization energy
Measures energy required to remove an electron from the atom (opposite of affinity)
28
Definition of a polarizability
Extent to which an electron cloud of an atom can be distorted by an external charge or by an applied electric field to produce a dipole
29
First IE definition
Removal of the first electron
30
Second IE definition.
Removal of the second electron
31
What takes more energy to remove an electron: valence electron or core electron?
Core electron ( metal have lower IE energy than nonmetals)
32
STP numbers are
0 C or 273 K
1 atm
1 mol of gas = 22.4 L
33
Positron emission is what type of decay?
Beta + decay
34
When the atoms are more stable?
When they have a full outer orbital shell
35
What properties share elements in the same column?
Just chemical (valence configuration)!!
Not physical (diff number of neutrons)!!
36
Nuclear fission definition
Splitting of a large atomic nucleus into multiple smaller nuclei
37
Isotope definition
Atoms share the same atomic number but different mass number( neutrons, density), same chemical properties but not physical
38
No polar means
EN less than 0.5
39
Polar means
EN from 0.5 to 1.7
40
Ionic bond means
Nonmetal plus metal, attraction of opposite charges.
Differences in electronegativity greater than 1.7
41
Covalent bond means
Electrons are shared between atoms
42
More electronegative atoms means that it has
Stronger attraction, valence electrons closer to the nucleus and less core electrons
43
As bond order increases then its bond strength
Increases, bond energy increases but bond length decreases
44
Relationship between atomic radii and bond length
More atomic radii has more bond length
45
As IE decreases the number of core electrons … which results
Increases and the noble gas is more stable as less attraction to the nucleus
46
As the size of an atom increases the polarizability …
Increases as well
47
Energy of a photon is directly proportional to … but inversely to …
its frequency
To its wavelength
48
Bohr model
Farther orbits = higher energy = shortest wavelength
Photon emitted when n decreases and absorbed when n increases
49
Empirical formula means
Ratio of each type of atom
By moles
50
Molecular formula means
Actual number of each type of atom
51
Structural formula means
How the atoms are bobsled to one another
52
In isoelecteonic atoms ionic radii decreases when
Atomic number increases
53
Size of anions and cations
Anions are bigger than cations
54
Combustion reaction definition
55
What diatomic atom makes a single bond?
H2, F2, Cl2, Br2, I2
56
What diatomic atom makes a double bond?
O2
57
What diatomic atom makes triple bond?
N2
58
Electrical conductivity tendency
Metals are the most vindictive then metalloids and then no metals( least conductive)
59
Valence shell diagram
60
Higher IO then reactivity is
Lower
61
Representative elements on the table are
s and p block ( groups 1-2, 13-18)
62
Reactivity of alkaline metals increases when
Atomic number increases
63
Oxidation definition
Reducing agent gives up electrons ( increases at the product)
64
Reduction definition
Oxidizing agent takes electron (decrease in products)
65
Concentration ratio
Stock solution/ standard solution
66
Dilution factor
Volume of the diluted solution/ volume of original solution
67
What happens during gamma emission?
Unstable nucleus in an excited state released excess energy by emitting a gamma ray which is a high energy photon without ejecting a particle
68
Orbital angular momentum quantum number
l (sub shell type: s, p, d or f)
Describes shape of the orbital where l = 0,1,2,3… (n-1)
69
Magnetic quantum numbers
ml determines number of orbitals and their orientation
All ranges from -l to +l
70
Electron spin quantum number
Ms angular momentum of an electron 1/2 spin up or down
71
Adding an electron is easier for what group?
Nonmetals
72
Why are noble gases the least reactive group?
They have a full valence shell configuration (full s and p except for He-only full s)
73
Reactivity of the atom means
Tendency to gain, lose or share electrons
74
Smaller atomic radius makes a bond
Stronger and smaller
Making it a weak acid
75
Large atomic radius makes bond to be
Longer and more acidic
76
Small electron affinity means
Increases electron electron repulsion between valence electrons
77
The most electronegative atom has an increased electron density creating a
Dipole
78
Lewis base is .. while Lewis acid is..
An electron donor,
Electron acceptor
79
Arrhenius base is a … while an acid is..
OH- donor, H+ donor
80
Brønsted-Lowry acid is a … while a base is a..
H+ donor, H+ acceptor
81
Metals ions in coordination chemistry act as
Lewis acids
82
Lewis based in coordination chemistry are
Ligands that coordinate with the metal ion
83
Heisenberg uncertainty principle definition
Exact position and momentum can’t be known both at the same time, just one of them where electrons in coordination bonds can be described only as probability distributions
84
Pauli exclusion principle
Two electrons in the same orbital must have opposite alignment
85
Types of magnetism
86
Control group is one that
Absent of independent variables
87
Contrast agent definition
Increase mri signals by increasing the relativity of water molecules to monitor biological processes
88
Atom can absorb a single photon with an energy equal ..
To the energy difference between the two states
89
Third IE is higher than the second IE because
It needs to remove a core electrons meaning it requires more energy to remove the electron as it tightly held
90
S orbital electrons requires more energy than p orbital because
It holds tightly therefore requires more energy to remove the electron
91
Dipole characteristics and types
Consists of opposite electric charges separated across a distance. In molecules, permanent dipoles form across some covalent bonds due to unequal sharing of electrons between two atoms caused by large differences in electronegativity. In a dipole, region with greater electron density gains (higher electronegativity between atoms) a partial negative charge while with less electron density ( higher electronegativity) positive charge.
Types: dipole-dipole - when the opposite charges of the polar bonds form a mutual attraction. Ion - dipole interaction - full charge of ion attracts the opposite charge of a polar bond dipole.
Dipole induced interaction - dipole form the polar bond distorts the electron cloud of a nonpolar bond and induced a weak attraction. London forces - form when two nonpolar bonds induce momentary dipole.
92
Electrolytes and compounds conductivity characteristics
Electrolyte - are solute that enable the conduction of electricity within a solvent (like NaCl).
Ionic compounds (metal + nonmetal) are conductive in liquid form but not in solid.
Metallic compounds - conductive in both solid and liquid states and have a high MP.
Molecular compounds - covalently bonded nonmetals and not conductive in both states.
93
Balanced net ionic equations conserve both …
Number of atoms and the net charge
94
Theoretical yield definition
Maximum amount of product that can form if all the limiting reactant is converted into products.
The amount of product that can be isolated from a fraction cannot exceed the theoretical yield.
The actual yield is always less than the theoretical because no reaction is perfect due to loss.
95
Double replacement reactions
Two compounds form two new compounds (ion swap)
96
Single replacement reaction
With a free element.
97
Ligand exchange via a … but their … are unchanged
Coordinate bond, oxidation numbers
98
Methods to test proposed mechanisms are
Certifying the reactions rate law,
Detecting an intermediate, interfering with a mechanistic pathway.
Having the same leaving groups is not a method !!!
99
Dipole moment is
u = qr where q- magnitude of the partial charge (increased when the the difference in electronegativity between two atoms increased and vice versa) and r - distance
