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139 Cards in this Set
- Front
- Back
_____ and ____ of atoms provide the theoretical foundation for the periodic classification |
Aufbau principle, electronic configuration |
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The elements in ____ exhibit similar ____ behaviour. |
Group, chemical |
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The similarity arises because the elements have the ______ and ______ of electrons in their outermost orbitals |
Same number, same distribution |
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Helium belongs to ______ block but is positioned in the ______ . |
S, p |
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On what basis hydrogen is similar to alkali metals |
Has only one s electron |
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On what basis hydrogen is similar to group 17 family |
To achieve noble gas arrangement can gain an electron |
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Give the atomic number of rubidium |
37 |
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Give the atomic number of caesium |
55 |
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Give the atomic number of francium |
87 |
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S block elements are all ____ with _____ ionization enthalpy |
Reactive metals, low |
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The reactivity _____ as we go down the group |
Increases |
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S block elements are never found in ____ owing to their _____ . |
Pure state, high reactivity |
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S and p block elements together constitute _____ elements or _____ elements |
Representative , main group |
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In p block the non metallic character ____ as we move from left to right across a period |
Increases |
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The D Block Elements have general electronic configuration of _____ |
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All D block elements are _____ |
Metals |
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The lanthanoids starts from _____(____) to ___ ( ____) |
Ce(Z=58), Lu(Z= 71) |
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The actinoids start from _____ ( ___) to ____(___) . |
Th(Z=90), Lr( Z= 103) |
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The electronic configuration of f block elements are |
(n-2) f1-14(n-1) d0-1 ns2 |
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The last electron in F block elements added to each element is filled in |
F orbital |
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F block elements are all |
Metals |
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The chemistry of _____ is more complicated than the corresponding lanthanoids, due to the large number of oxidation States possible |
Early actinoids |
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Many of the actinoid elements have been made only in _____ quantities or even less by nuclear reactions and their chemistry is _____ fully studied |
Nanogram, not |
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Elements after uranium are called |
Trans uranium elements |
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The electronic configuration of Z =117 |
(Rn) 5f14 6d10 7s2 7p5 |
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Electronic configuration of Z = 120 |
(Uuo) 8s2 |
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Metals comprise more than ____ of all known elements and appear on the ____ side of periodic table |
78%, left |
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______ And ____ also have very low melting points |
Gallium, caesium |
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By ____ property metals can be flattened into thin sheets by hammering |
Malleable |
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By _____ property metals can be drawn into wires |
Ductile |
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Non metals are usually solids or gases at room temperature with ____ melting and boiling points |
Low |
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Non metals are _____conductors of heat and electricity |
Poor |
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Most non metallic solids are ___ and are neither malleable nor ductile |
Brittle |
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The change from metallic to non metallic character is not ____ |
Abrupt |
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Give example of semi metals |
Silicon , Germanium , arsenic, antimony , tellurium |
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Si, Be, Mg, Na, P : Order of metallic character is |
Na>Mg>Be>Si>P |
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In non metals the reactivity ____ down the group |
Decreases |
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The measurement of the distance between two atoms when they are bound Together by a _____ bond in _____ molecule forms the covalent radius. |
Single, covalent |
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______ Is taken as half the inter nuclear distance separating the cores |
Metallic radius |
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Noble gases are ____ . |
Monoatomic |
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Noble gases have ____ radii. |
Van der waal |
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Noble gases have _____ radii |
Non bonded |
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The ionic radii can be estimated by measuring the distance between cations and anions. T/F. |
T |
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The Ionic radius of fluoride ion is ____ where as the atomic radius of fluorine is only _____ . |
136 pm, 64 pm |
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In the ionic form the radius of the metals or nonmetals generally decreases or increases by a factor of |
2 |
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In isoelectronic Species the radii would be ____ |
Different |
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The energy required to remove an electron from an isolated gaseous atom in its ground state is |
Ionization enthalpy |
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Energy is always required to ____ electrons from an atom and hence ionization enthalpy are always _____ . |
Remove, positive |
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In the graph of ionization enthalpy ____ occupy the maxima and _____ occupy the minima |
Noble gases, alkali metals |
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Why alkali metals occupy the minimum position in the ionization enthalpy graph |
Due to their low ionization enthalpy |
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Shielding is effective when the orbitals in the inner shells are ____ . |
Completely Filled |
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Down the group increase in ____ outweighs the increasing _____ so removal of outermost electron requires ______ energy down the group |
Shielding, nuclear charge, less |
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The penetration of ____ electron to the nucleus is more than that of ____ electron. |
2s, 2p |
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In oxygen atom ____:of the four ____ electrons must occupy the same ____ orbital resulting in an increased ___ repulsion |
2, 2p, 2p, electron - electron |
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Due to ______ it is ___ to remove the fourth 2p electron from oxygen in comparison to nitrogen |
Electron electron repulsion, easier |
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Ionization enthalpy _____ across the period |
Increases |
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Electron gain enthalpy provides a measure of the ease with which an atom ____ an electron to form _____ . |
Adds, anion |
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For many elements energy is _____ when an electron is added to the atom and the electron gain enthalpy is ______ . |
Released, negative |
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Halogens have ______ electron gain enthalpy because they can attain stable electronic configuration by _____ electron. |
High negative, adding one |
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Noble gases have _____ electron gain enthalpy because the electron has to enter the next higher _____ level leading to very unstable electronic configuration |
Large positive, principle Quantum, |
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The electron gain enthalpies have ________ values toward the upper right of the periodic table preceding the noble gases |
Large negative, |
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As a general rule electron gain enthalpy becomes _____ with increase in atomic number across a period |
More negative |
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Cl has -349 ∆Hege . What does negative sign means |
When an electron is added to the atom enthalpy is negative |
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Cl has -349 ∆Hege. What does the magnitude represent |
The high magnitude represents the tendency to gain electron |
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What is the general rule which can be applied for electron gain enthalpy |
Enthalpy is negative when an electron is added |
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When does an atom has positive electron gain enthalpy |
When it does not want to add electron , eg: noble gas |
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The positive and electron gain enthalpy indicates |
The tendency with which an electron is repelled |
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The high value of electron gain enthalpy indicates |
Height of Desire |
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The effective nuclear charge ____ from left to right across a period |
Increases |
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Due to increased effective nuclear charge it will be ____ to add an electron to _____ atom because the added electron on an average would be closer to the positively charged _____ |
Easier, smaller, nucleus |
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Electron gain enthalpy becomes _____ as we go down a group |
Less negative |
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The electron gain enthalpy of oxygen or fluorine is ______ than that of the succeeding element because of significant ____ . |
Less negative, repulsion |
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The negative of electron gain enthalpy is defined as |
Electron affinity |
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Electron affinity is defined as |
Absolute zero |
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Give the relation between electron gain enthalpy and electron affinity |
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Electronegativity is a _____ measure |
Qualitative |
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Electronegativity is a measurable quantity. T/F |
F. Electronegativity is not a measurable quantity |
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Mulliken-Jaffe scale is applicable to _____ |
Electronegativity |
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Allred - Rochow scale is related to |
Electronegativity |
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Why does the magnitude of electron gain enthalpy decreases down the group |
Because down the group the size of the atom increase and the added electrons would be farther from the nucleus |
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The magnitude of electron gain enthalpy ______ down the group |
Decreases |
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The electronegativity of any given element is _____ . |
Not constant |
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Electronegativity depends on the ____ to which it is bound |
Element |
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Elements have constant electronegativity |
False |
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Electronegativity is a measurable quantity |
False |
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Electronegativity is not a _____ quantity |
Measurable |
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_____ provides a mean of predicting the nature of force that holds a pair of atoms together |
Electronegativity |
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The electronegativity of any given element is |
Variable |
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Electronegativity generally increases across a period from |
Left to right |
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Electronegativity value _____ with the increase in atomic radii down a group. |
Decreases |
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The trend of electronegativity is similar to |
Ionization enthalpy |
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Electronegativity is directly related to _____ property of the element |
Non metallic |
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Electronegativity is ______ related to the metallic properties of elements |
Inversely |
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Increase in electronegativities across a period is accompanied by _______ in non metallic properties |
Increase |
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Decrease in electronegativities down a group is accompanied by |
Increase in metallic properties |
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Give the electronegativity of |
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Give the electronegativity of |
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Give electronegativity of |
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Give electronegativity of |
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The _____ is the most characteristic property of the element |
Valence |
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In OF2 molecule oxygen ____ two electrons with fluorine atoms |
Shares |
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Oxidation state is defined as the charge acquired by its atom on the basis of _____ consideration from other atoms in the molecule |
Electronegative |
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Give the number of valence electron |
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Give the valence of |
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There are many elements which exhibit variable valence. This is particularly characteristic of _____ elements and _____ . |
Transition, actinoides |
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Lithium shows diagonal relationship with |
Magnesium |
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Beryllium shows diagonal relationship with |
Aluminium |
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The maximum covalency of the first member of each group is |
4 |
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The first member of p block elements displays greater ability to form _______ multiple bonds to itself and to the other ___ period elements. |
Pπ-pπ, second |
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Give the order of metallic radius of Lithium and magnesium |
Mg>Li |
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Give the order of Ionic radius of Lithium and magnesium ion |
Li+>Mg+ |
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The chemical reactivity at the two _____ is highest and the lowest in the _____ . |
Extremes, centre |
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The metallic character ___ while the non metallic characters ____ while moving from left to right across the period |
Decreases, increases |
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Oxides of elements in the centre are ____ or ____ |
Amphoteric , neutral |
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As2O3 is _____ in nature |
Amphoteric |
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Give example of neutral oxides |
CO NO N2O |
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Give the nature of N2O |
Neutral |
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Transition metals are _____ electropositive than first and second group metals |
Less, |
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Who was the first to consider the idea of trends among properties of elements |
Johann dobereiner |
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Give the group one triad of Dobereiner's triad |
Li Na K |
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Give the group two triad of Dobereiner's triad |
Ca Sr Ba |
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Give the group 17 triad of Dobereiner's triad |
Cl Br I |
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What comment did the dobereiner passed on the triads |
Properties of the middle element was in between those of the other two members |
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Who arranged the then known elements in order of increasing atomic weights |
Chancourtois |
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Who made a cylindrical table of elements to display the periodic reference of properties |
Chancourtois |
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Law of triods was given in |
Early 1800s(1829) |
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Law of octaves was given in |
1865 |
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Who gave law of octaves |
Newland |
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Law of octaves seemed to be true only for elements up to |
Calcium |
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Who was awarded the davy medal in 1887 |
Newland |
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Dimitri mendeleev |
1834 to 1907 |
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Lothar Meyer |
1830- 1895 |
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Who is generally credited with the development of modern periodic table |
Dimitri mendeleev |
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Who plotted various physical properties against atomic weight to obtain a periodically repeated pattern |
Meyer |