Fill in the blanks with the relevant term or words.
1. Dalton stated: All atoms of an element are alike in ______mass_______and other
properties, but the atoms of one element are _____different__________ from those of
all other elements.
2. According to the Dalton’s statement, each chemical element is composed of minute,
indestructible particles called ____atoms_____.
3. In each of their compounds different ____elements______combine in a simple
numerical ratio.For example one atom of A to one of B(AB), or one atom A to two of
B(AB2)
4. Faraday discovered_____ cathode rays ________, a type of radiation emitted by the
negative terminal cathode that crossed the evacuated tube to the positive terminal or
____ anode.___
5. _______ Fluorescence ________is the term used to describe the emission of light by
a material when it is struck by energetic radiation.
6. In 1897, Thomson established the ratio of ____ mass to electric charge
(m/e)_______
7. Millikan determined______ the electronic charge e _____ through a series of oil
drop experiments
8. In 1895, Wilhelm Roentgen discovered ____X rays_____ , a type of electromagnetic
radiation in the invisible region and which he called so because of its unknown nature.
9. ___Radioactivity_____ is the spontaneous emission of energy from unstable atoms.
10. ____Radioactive decay_____ is the process by which an atomic nucleus loses its
energy by emitting ionizing particles
11. _______ Alpha particles ____ carry two fundamental units of positive charge and
have the same mass as helium atoms. They have +2 charges.
12. ______ Beta particles________are negatively charged particles produced by changes
occuring within the nuclei of radioactive atoms and have the same properties as
electrons.
13. _____Gamma rays _____are defined as the electromagnetic radiation of extremely
high penetrating power.
14. When the radiation is passed through the electric field, ___ gamma rays ______ are
undeflected. ____________ Alpha particles and beta particles ________are
deflected in the opposite directions of each other.
15. Most of the mass and all of the positive charge of an atom are centered in a very small
region called the ____ nucleus.________
16. The sum of the protons and neutrons located in the nucleus of an atom is defined as
___nucleon____.
17. Elements beyond _______ uranium (Z=92)_______do not occur naturally and must
be synthesized in particle accelerators .
18. Two or more atoms having the same atomic number (Z) but different mass numbers
(A) are called _____ isotopes ________
19. The device used for measuring the isotopic masses of each element is called
___________mass spectrometry______________
20. The greater the _________principal quantum number_______________, the farer
the shell from the nucleus.
21. _______________Angular momentum quantum number________determines the
geometrical shape of the electron probability distribution.
22. Each subshell is composed of one or more _____ orbitals ______and each orbit in a
sub-shell is defined as ___magnetic quantum number______“ml”
23. ___________ Spin magnetic quantum number, ms________ indicates the direction
of an electron found in an orbital present in a magnetic field.
24. Electrons that are added to the electronic shell of highest principal quantum
number(the outermost shell) are called _______valence electrons_____
25. Metals are good conductors of ____heat________ and _____electricity__________.
26. Nonmetals build up _____ covalent ___________bonds among each other, and form
______ ionic ________bonds with metals and metalloids
27. _____Metalloides_____ are elements that look like metals and in some way behave
like metals, but that also have some nonmetallic properties
28. The element or ions which have the same number of electrons are called
_____isoelectronic______
29. The more easily an atom ____ loses____its ___ electrons____, the more it tends to
have a metallic character.
30. ___ Ionization Energy _____is the quantity of energy a gaseous atom must absorb so
that an electron is stripped from the atom.
31. Ionization energies ___ decrease ____as atomic radii increase.
32. ___ Electron affinity _____, is a measure of the energy change that occurs when a
gaseous atom gains an electron .
33. The elements of ___Group VIIA_____ have the highest negative electron affinities
in the periodic table.
34. ___ The IIA and VIIIA group elements_______ have positive electron affinities
because the electron gained must enter the higher energy orbital since all the other __
s and p__ orbitals of the atoms are filled. This situation requires an ____
endothermic _____process.
35. The oxides of metals have __basic_____ character, but the oxides of nonmetals have
__acidic____ character.
36. The elements found in Group 8A are called __noble gases___.They are at
__gaseous__ state at room temperature.
37. ___The transition elements_____ are d block and f block elements of the periodic
table.
38. In the series of the first inner transition elements elements in which the __4f__
subshell is filled,atomic sizes actually decreases somewhat. This phenomenon is
called ___ lanthanide ___ contraction.
39. The transition elements have __ionic__ character in low oxidation states and
___covalent___ character in high oxidation states.
40. Fe, Co and Ni are ___ ferromagnetic ____which means that the magnetic moments
are aligned into domains. The ordering of domain persists when the object is removed
from the magnetic field and thus permanent magnetism results.
41. Standard electrode potentials of the transition elements __ increase___ in value across
the series. All these elements except for __Copper_are more readily oxidized than
hydrogen.
42. The group IA elements are called ___alkali metals____. Each of them has __1____
electron in their outermost s orbital. They are the group having the smallest ___first
ionization energy____ among the other groups of elements in the periodic table.
43. Group IIA elements are called __alkaline earth metals___. Compared to Group IA
elements, they have higher ___densities___ and __melting points_____
44. ___Chemical compounds_____ are composed of two or more different elements
45. A __ molecule ____of a compound is a group of bonded atoms that actually exists and
can be identified as a distinct entity
46. ___ Chemical formula ___indicates the elements present and the relative numbers of
atoms of each element in the compound
47. The ___ ionic compounds ___are the compounds comprised of positive and negative
ions joined together by electrostatic forces of attraction.
48. As a result of the electron transfer, the metal atom becomes a positive ion and is a___
cation___. And the nonmetal atom becomes a negative ion and is called an ___
anion__.
49. ___ Oxidation state ___designates the number of electrons that an atom loses, gains
or otherwise uses in joining with other atoms in compounds.
50. The compounds in which the water molecules are incorporated in the solid structure of
the compound are called ___hydrates___
51. Liquid pressure depends only on the ___height___ of the liquid column and the
___density____ of the liquid.
52. The device used to measure the atmospheric pressure is called __barometer___
53. The device used to measure the pressure of a gas in a closed vessel is called
___manometer___
54. Gas densities depend strongly on temperature and pressure; __ increasing__ as the
gas pressure increases, ___ decreasing __as the temperature increases.
55. The density of a gas is directly proportional to its __ molar mass___.
56. The ratio of partial volume to total volume, or of partial pressure to total pressure is
the ____mole fraction____.
57. The kinetic energy of gaseous molecules is a function of ____temperature_______.
The rate of ____diffusion________ of two different gases are inversely proportional
to the square root of their molecular mass.
58. The rate of diffusion of two different gases are inversely proportional to the square
root of their _____molecular masses________
59. The escape of gas molecules from their container through a tiny orifice or pin hole is
called ____effusion_____
60. The migration of molecules of different substances as a result of random molecular
motion is called ___diffusion____
61. At very high pressures and low temperatures gases tend to behave as
___nonideally______, which can be explained with the concept
_______compressibility factor____________(PV/nRT > 1)
62. At very low pressures and high temperatures gases tend to behave as
___ideally______
63. If there is no possible transfer of energy and or matter between the system and its
surroundings, the system is called ___isolated______
64. If there is only free transfer of energy between the system and its surroundings, it is
called a ___closed____ system.
65. Heat transfer between the system and its surroundings occurs as a result of ___
temperature _____ difference.
66. The heat flux occuring at constant temperature is called ____ isothermal
process____.
67. The quantity of heat energy ,q , depends upon the change in __temperature___ , the
___quantity___ and ___nature____ of substance
68. The pressure-volume work in gases (P ΔV= w) has a positive sign (+), when work is
done _on__ the system.
69. The pressure-volume work in gases (P ΔV= w) has a negative sign (-), when work is
done _by__ the system.
70. An ___endothermic_____ reaction gains heat from the surroundings (ΔH > 0)
71. An ___exothermic________ reaction delivers heat to the surroundings (ΔH < 0)
72. The quantity of heat required to change the temperature of a system by one degree is
called ____heat capacity__________(mass x specific heat)
73. The type of calorimeter called __bomb calorimeter____ is ideally suited for
measuring the heat evolved in the combustion reaction.
74. In interactions between a system and its surroundings, the total energy remains ___
constant___
75. The device working under constant pressure and used to measure the quantity of heat
in an isolated system composed of a styrofoam cup is called ___coffee cup
calorimeter____
76. In thermodynamics __ work____ means the transfer of energy between the system
and its surroundings due to an external makroscopic force.
77. Apart from transfer of heat, some chemical processes may do work.(for example: the
___expansion or ___compression___ of gases)
78. A system does not contain energy in the form of heat or work. It keeps the energy in
form of ___internal energy__ (U)
79. The change in the internal energy of an isolated system is equal to ___0____
80. If, on balance more energy enters the system than leaves, ΔU is ___ positive___.If
more energy leaves than enters, ΔU is __ negative___.
81. At constant pressure and temperature ___ H___ = U + PV
82. Standard molar enthalpy of formation(molar heat of formation), Hf is the
difference in enthalpy between one mole of a compound in its standard state and its
elements in their most stable forms and standard states.
83. Since enthalpy change is directly proportional to the ___ amounts___of substances in
a system, it is an ___ extensive___ property of matter.
84. H of a chemical reaction changes sign when a process is ___ reversed___.
85. We assign enthalpies of __ zero___ to the elements in their most stable forms when
in the standard state.
86. The component that is present in the greatest quantity or that determines the state of
matter in which the solution exists is called __solvent___
87. A solution component that is present in a solution in lesser quantity than the solvent is
called ___solute___
88. Solutions containing a relatively high concentrations of solute are called
___concentrated____
89. Solution containing a relatively low concentrations of solute are called ___diluted___
90. Solid solutions with a metal as the solvent ; e.g. brass (Cu-Zn), solder (Sn-Pb) are
called __alloys___
91. ___ Mercury in gold ____is a good example for solid solvent and liquid solute
mixtures
92. ___ Pt/H2 ____is a good example for solid solvent and gaseous solute mixtures
93. ___ Alcohol in water ____is a good example for liquid solvent and liquid solute
mixtures
94. ___ Mineral water ____is a good example for liquid solvent and gaseous solute
mixtures
95. ___Molality___ is defined as the ratio of nsolute to the amount of solvent(msolvent)
96. ___Molarity___ is defined as the ratio of nsolute to the volume of solution(Vsolution)
97. If all intermolecular forces of attraction are of about equal strength, a random of
intermingling of molecules occurs. A homogenous mixture or solution results and this
is called as ___ ideal solutions____.
98. ___ Benzene- Toluene___ mixture is a good example for ideal solutions
99. If forces of attraction between same molecules, A-A or B-B (molecules between
solvent or solute), are SMALLER, than forces of attraction of unlike molecules A-B,
(forces between solute and solvent), a solution is formed but its properties can not be
predicted. These are identified as ___ non-ideal solutions___.
100.
___ Chloroform-acetone ___is a good example for non-ideal solutions
101.
If forces of attraction between same molecules, A-A or B-B (molecules
between solvent or solute), are MUCH GREATER, than forces of attraction of unlike
molecules A-B, (forces between solute and solvent), dissolving does not occur to any
siginificant extent. The components remain segregated in a __ heterogenous___
mixture.___Water-octane____ is a good example for these mixtures.
102.
When the solute and the solvent are mixed up; First dissolving occur, Then
precipitation starts and increases with time. After a while the dissociation and
precipitation rates become equal. The quantity of dissolved solid remains constant
with time. These solutions are called ___saturated___
103.
The concentration of the saturated solution is called the ___ solubility __of
the solute in the given solvent and it varies with temperature. It can be expressed as
Molarity or ___ Mass Percent____
104.
KNO3 dissolves in 100 g water and 30oC at an amount of ~32g . At the same
temp., if 30g KNO3 are dissolved, it is __ unsaturated__, 35g KNO3 are dissolved, it
is__ supersaturated___
105.
The solubilities of some ionic substances such as SO32-, SO42 ___decrease___
with increasing temperature.
106.
When ___Hsoln > 0____, raising the temperature increases the solubility.
107.
When ___Hsoln < 0____,the solubility decreases with increasing
temperature.
108.
We prepare a concentrated solution at a high temperature. Then we let the
solution cool. At lower temperatures the solution becomes saturated in the desired
compound. The excess compound crystallizes from solution and the impurities remain
in solution. This method of purifying a solid called ____ fractional
crystallisation____
109.
The solubility of a gas increases as the gas __ pressure___is increased. This is
called Henry’s law.
110. The solubilities of gases __ decrease ___with increased temperature
111. The partial pressure exerted by solvent vapor above an ideal solution, PA, is the ___
vapor pressure___ of the pure solvent at the given temperature PAo, multiplied by the __
mole fraction___ of the solvent in the solution, XA
112. In nonideal solutions, if the departures from ideal solution behaviour are sufficiently
great, certain solutions may vaporize to produce a vapor that has the same composition as
the liquid. These solutions, called ___ azeotropes____ boil at a constant temperature and
because the liquid and vapor have the same composition, they can not be seperated by
fractional distillation
113. The properties such as _Vapor pressure lowering, ______freezing point
depression____, ____ boiling point elevation _____,________ and ___osmotic
pressure___ whose values depend only on the concentration of solute particles in
solution and not on what the solute is, are called colligative properties.
114. The necesssary pressure to stop osmotic flow is called the ___ osmotic pressure___
and represented by the symbol Π.
115. By means of ______reverse osmosis__________, pure water can be obtained from
seawater and other waste water can be reused by this way.
116. To lower the freezing point of water and to deice roads, ___salt___ is used.
117. Ethylene glycol is an ___antifreezing__ agent used to prevent the car engines from
freezing.
118. For chemical reactions, ___rate of reaction____ describes the change in
concentration of a reactant or product with time.
119. For a given chemical reaction, the rate of reaction is as follows:
R= k [A]2 [B]-1, where A and B are the reactants. The overall order of reaction is
___1__
120. For a given chemical reaction, the rate of reaction is as follows:
R= k [A]2- [B] [C], where A , B and C are the reactants. The overall order of reaction
is ___0__
121. In a __zero___ order reaction, the concentration-time graph(plotted above) is a
straight line with negative slope which shows the ___rate of reaction______
122. The ___half-life_____ of a reaction is the time required for one half of reactant to be
consumed.
123. In a chemical reaction, the value of the ___rate constant___ depends on the type of
reaction, type of catalyst and temperature
124. The unit of the rate constant depends on the ___order___ of reaction.
125. Chemical equilibrium is ___dynamic____ because it can move in two directions
either forward or reverse according to the effect exerted onto the reaction
126. Within the natural events, it is the deal point of having the tendency of longing to
have either minimum ____enthalpy____ or maximum ___entropy____.
127. The ___vapor pressure_____ of a liquid is a property associated with an equilibrium
condition.
128. ___The solubility___ of a solute is a property associated with an equilibrium
condition.
129. The ____distribution_____ coefficient of a solute between two immiscible solvents is
a property associated with an equilibrium condition.
130. The concentrations terms for pure ____solids___ and___ liquids____ do not appear in
equilibrium constant expressions.
131. If an ___inert____ gas is added into a constant volume of a reaction mixture, it will
have no effect on the equilibrium condition.
132. Raising the temperature of an equilibrium mixture shifts the equilibrium condition in
the direction of the ____endothermic____ reaction.
133. Lowering the temperature causes a shift in the direction of the ___exothermic____
reaction
134. A ___catalyst___ in a reaction mixture speeds up both the forward and reverse
reactions but it does not change the equilibrium amounts.
135. When a strong acid and a strong base react with each other, ___salt___ and
__water____ are produced.This reaction is called ___neutralization____ process.
136. According to the Bronsted_Lowry theory an acid is a proton ___donor___ and a base
is a proton ___acceptor____
137. The Bronsted-Lowry theory accounts for substances that can either react as an acid or
a base; they are said to be ___amphiprotic____.
138. If the pH is less than 7, the solution is ___acidic____, if the pH is greater than 7, the
solution is ____basic____
139. ___Percent ionization___ gives the proportion of ionized molecules.
140. The percent ionization of a weak acid or a weak base increases as the solution
becomes more ___dilute___.
141. Some acids have more than one ionizable H atom per molecule. These are called
____polyprotic____ acids.
142. There are some water solutions, called ___buffer____ solutions, whose pH values
change only very slightly upon the addition of small amounts of either an acid or a base.
143. Common buffer solutions are described either as a mixture of a ___weak___ acid and
its conjugate ___base___ or a ___weak__ base and its conjugate___ acid____
144. An __ acid-base indicator___ is a substance whose color depends on the pH of the
solution to which it is added.