Chemistry Flashcards
Smallest subdivision of an element that can take part in a chemical reaction
Atom
Smallest subdivision of an element or a compound that can exist in a free state
Molecule
Electrons in the outermost orbit
Valence Electrons
Approximately equal to the sum of the number of neutrons and protons in the nucleus
Atomic mass
Equal to the weighted average of all the masses of the isotopes
Atomic mass
Equal to the number of protons in the nucleus
Atomic Number
What orbital is the most stable state that an electron can occupy
S orbital
As you move from left to right the Atomic Weight ________.
Increases
The Vertical columns in a periodic table are called?
Groups/Families
How many total groups/families in the periodic table?
18 columns
How many columns are in the main groups of the periodic table?
8 columns
How many columns in the transition metal groups?
10 columns
How many periods are there in the periodic table?
Seven (7)
It is the tendency to absorb electrons from neighboring atoms.
Electronegativity
Negatively charged ions.
Anions
These are types of ions that lose its electrons at the anode during electro-chemical reaction.
Anions
An anion becomes negatively charged because it _________ an electron. (Hint: absorb, release)
Absorbs
In order to become neutral, an Anion must ________ electron.
release
What do you call the loss of an electron in an ion?
Oxidation
The charge/no. of electrons absorbed by an ion from neighboring atoms.
Oxidation number
This refers to the number of electrons that must be lost to achieve charge neutrality.
Oxidation number.
When an atom loses an electron it becomes ________ charged.
Positive
These are the positively charged ions
Cations
These ions gains electrons and are formed at the cathode in electro-chemical reaction.
Cations
Cations must _______ electrons to become neutral
Gain
This refers to the gaining of an electron by an atom/ion
Reduction
Also called Electrovalent Bonding
Ionic Bonding
The type of linkage or bonding formed from the electrostatic attraction between oppositely charged ions
Ionic Bonding
This type of bonding is formed between atoms of high electron affinities and low ionization energies.
Ionic bonding
This refers to sharing of electrons
Covalent Bonding
The type of bonding common in gases that form diatomic molecules in their free state.
Covalent bonding
This type of bonding occurs in elements with same electron affinity and ionization energy.
Covalent Bonding
This type of bond is typical in organic compounds
Covalent Bonding
Simplest type of Chemical reaction where two elements or compounds combine directly to form a new one.
Direct Combination / Synthesis
Another name for the Direct Combination chemical reaction.
Synthesis
In this type of Chemical reaction, the bonds uniting a compound are disrupted by heat or another energy source to yield simpler compounds or elements.
Decomposition
This type of Chemical reaction is identified by one element and one compound as the reactants
Single Displacement
This type of chemical reaction is characterized by having two compounds as reactants and forming two new compounds
Double displacement
This type of reaction involves oxidation of one substance and the reduction of another.
Oxidation - Reduction
Study of proportions in which elements combine into compounds
Stoichiometry
This refers to the no. of gram equivalent weights of solute per liter of solution
Normality
Refers to the no. of grams mole per liter of solution
Molarity
Refers to the gram formula weights per liter of solution
Formality
Refers to the no. of gram moles of solute per 1000 grams of solvent.
Molality
Refers to the no. of moles of solute divided by the no. of moles of solvent and all solutes
X mole fraction
These are any substance/s that dissociates in water into H+ or H3O+
Acids
These substances dissociates in water and gives up OH-
Bases
Charge in an electron
- 1.6 x 10^-19 C
Charge in a proton.
+1.6 x 10^-19 C
Weight of an electron
9.109 x 10^-31 kg
1 amu = ________ kg
1.67 x 10^-27 kg
1 amu = ______ g/mol
1 g/mol
It is equal to the number of molecules per element in a compound multiplied with amu.
Molecular Mass/Weight
1 mole = _______ atoms/molecules
Avogadro’s Number (6.02 x 10^23 atoms/molecules)
Formula for percent composition of an element in a compound.
MW(element) / Sum of the total MW in the compound
In Ideal Gas Laws, the value of R to be used when you are given
L-atm/mol-K
0.0821
In Ideal Gas Laws, the value of R to be used when you are given
J/mol-K
8.314
Ideal Gas law variant where the Temperature is held constant.
Boyle’s Law
Formula for Boyle’s Law
P1V1 = P2V2
Ideal Gas Law variant where the Pressure is held constant.
Charles’ Law
Formula for Charles’ Law
V1/V2 = T1/T2
Ideal Gas Law variant where the Volume is held constant
Gay-Lussac’s Law
Formula for Gay-Lussac’s Law
P1/P2 = T1/T2
It states that the total pressure is equal to the sum of the individual Pressure of all the gases in a container.
Dalton’s Law of Pressure
Ideal Gas Law Variant where the Pressure and Temperature are held constant
Avogadro’s Law
Formula for Avogadro’s Law
V1/V2 = n1/n2
Formula for Ideal Gas Law
PV = nRT
Formula for Combined Gas Law
(P1V1)/(P2V2) = T1/T2
The mass of the proton with respect to the mass of the electron
Mp = 1836 Me-
The mass of the neutron with respect to the mass of the electron.
Mn = 1839 Me-
This refers to variants of an atom with same no. of protons but with different neutrons
Isotopes
Atoms with less than 4 valence electrons are _______?
Conductive
Atoms with 4 valence electrons are _________.
Semi-conductive
Atoms with more than 4 valence electrons are _______.
Insulating
As you move from Right to left, the Atomic Radius _______.
Increases
As you move from Top to Bottom, the Atomic Radius _________.
Increases
As you move from Left to Right, the Atomic Radius _________
Decreases
As you move from Bottom to the Top, the Atomic Radius ________
Decreases
As you move from Left to Right , the Ionization Energy _______
Increases
As you move from Bottom to Top, the Ionization Energy ________
Increases
As you move from Right to Left, the Ionization Energy ________
Decreases
What are the 7 Base SI units
m, kg, s, K, A, cd, mol
What are the 7 Diatomic Elements
H, N, F, O, I, Cl, Br
Have No Fear Of Ice Cold Beer
Value of the Standard Temperature
273 K
Value of the Standard Pressure
1 atm
It is the movement of gases from High Concentration to Low Concentration.
Diffusion
Formula for Rate of Diffusion.
Rate of Diffusion = (amount of gas passing an area) / (unit of time)
Movement of gas through a small opening
Effusion
The Volume of 1 mole of any kind of gas is?e
22.4 Liters
Elements in the Group 1A are called?
Alkali Metals
Elements in the Group 2A are called?
Alkaline Earth Metals
What are the 7 Metalloid Elements?
B, Si, Ge, As, Sb, Te, Po
What is the Atomic mass of Helium?
4
What is Atomic Mass of Lithium?
7
What is the atomic number and mass of Boron?
5, 10.8
What is the atomic mass of Carbon?
12
What is the atomic mass of Nitrogen?
14
What is the atomic mass of Oxygen?
16
What is the atomic mass of Fluorine?
19
What is the Atomic mass of Na?
23
What is the Atomic mass of Mg?
24.3
What is the Atomic Mass of Aluminum?
27
What is the atomic Mass of Si?
28
What is the atomic mass of P?
31
What is the atomic mass of Sulfur?
32
What is the atomic mass of Chlorine?
35.45
What is the atomic mass of K?
39
What is the atomic mass of Calcium?
40
What is the atomic mass of Chromium?
52
What is the atomic mass of Mn?
55
What is the atomic mass of Fe?
55.85
What is the atomic mass of Ni?
58.7
What is the atomic mass of Cu?
63.55
What is the atomic mass of Zn?
65.39
What is the atomic mass of Br?
80
What is the atomic mass of Ag?
108
What is the atomic mass of Iodine?
127
What is the atomic mass of Gold?
197
What is the atomic mass of Hg?
200.5
What is the atomic mass of Pb?
207.2
The Lanthanides and Actinide Series are also called what?
Inner Transition Metals
“When two or more elements form more than one compound, the ratio of the masses of one element that combine with a given mass of another element in the different compounds is the ratio of small
whole numbers.” This statement is known as:
Law of Multiple Proportion
This states that the rate of effusion of gas is inversely proportional to the square root of its molecular mass.
Graham’s Law
“The total pressure of a mixture of gases equals the sum of the partial pressures of each of the gases in the mixture”. This statement is known as __________.
Dalton’s Law of Partial Pressure
“At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.” An equivalent way of stating the law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid: This statement comes from_________?
Henry’s Law
__________ states that the lowest energy electron configuration, the ground state, in any electron subshell is the one with the greatest number of parallel electron spins.
Hund’s Rule
In the ____________ of acid-base reactions, bases donate pairs of electrons and acids accept pairs of electrons.
Lewis Theory
__________ states that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature scaled by the mole fraction of the solvent present:
Raoult’s law
“When the elements are arranged in the order of increasing atomic number, elements with similar properties appear at periodic
intervals.” This statement is known as _________.
The periodic law
This refers to the property of a material that is dependent on the amount of matter present.
Extensive Property
This refers to the property of matter that is dependent only on the type of matter present and not on the amount.
Intensive Property
It expresses the reaction rate in terms of changes in the concentration of one or more reactants (Δ[R]) over a specific time interval (Δt).
Differential Rate Law
