Trends which are observed in the properties of elements as you move along the periodic table in a given direction.

learn more… | top users | synonyms (1)

-1
votes
0answers
12 views

Confusion regarding periodic properties

Its said that inter electronic repulsion makes Cl-Cl bond length more than F-F.Is this also the reason for a stronger Cl-Cl bond than F-F?
1
vote
0answers
16 views

Relation of Boiling Point and Melting Point with the reactivity of an element

When we look at the trends of periodic table, there is an interesting correlation to be noticed. Along a period, when we look at the trends in reactivity of an element( Both due to electropositivity ...
0
votes
0answers
18 views

Why do alkali metals have negative electron gain enthalpy?

Alkali metals should have positive electron gain enthalpy as they are electropositive elements and also there atomic size is big in their periods so they should be reluctant to take electrons but they ...
4
votes
0answers
40 views

How to compare the oxidizing power of perhalate ions

In my book the oxidizing power in descending order of the following is given as: $\ce{BrO4-} > \ce{IO4-} > \ce{ClO4-}$ My doubt is regarding their order of oxidizing tendency. I thought that ...
0
votes
0answers
10 views

why is lithium the most electronegative element in its group [duplicate]

lithium has got the highest negative electrode potential in its group showing that it has the maximum tendency to donate an electron but still it has got the highest ionisation enthalpy
2
votes
0answers
15 views

Inert Pair Effect [duplicate]

My notes say that inert pair effect is the tendency of electron in the outermost atomic s orbital to remain unionised or unshared in compounds of post-transition metals. (Eg. Sncl2 is formed ...
1
vote
0answers
21 views

On the oxyacids of +III pnictogens and +IV chalcogens

Phosphorus in its $\mathrm{+III}$ oxidation state is known to exist as the phosphonic acid tautomer rather than phosphorous acid one. All salts isolated containing $\ce{H2PO3-}$ are (to the best of my ...
4
votes
1answer
81 views

Bond length increase when replacing nitrogen with phosphorus for NH3 and NF3

There is an increase in bond length of about $40\rm~pm$ from $\ce{NH3}$ to $\ce{PH3}$, but only by about $20\rm~pm$ from $\ce{NF3}$ to $\ce{PF3}$. I understand that the bond length will increase with ...
0
votes
0answers
22 views

Basic Screening effect concept

The sequence of shielding capacity by the electrons in different sub shell is given as s > p > d > f Along with it, if all sub shells are completely filled with electrons, the order of screening will ...
-1
votes
0answers
24 views

I need help to understand the reacitvity of a certain element.

I need help to understand the reacitvity of a certain element. I understand that phosphorus has a higher first ionisation enegy than silicon in period 3. However phosphorous reacts with oxygen gas ...
1
vote
2answers
59 views

Does increasing electronegativity imply more covalent character?

If there is a larger electronegativity difference between two atoms, shouldn't the compound be more ionic? In an explanation of the diagonal relationship, it states that "on moving across the period, ...
1
vote
0answers
37 views

Why Don't Sulfur Atoms Hybridize?

I am doing some chemistry problems with given answers, and supposedly the $107^{\circ}$ and $92^{\circ}$ bond angles in $\ce{H_2O}$ and $\ce{H_2S}$, respectively, is due to the fact that"$\ce{O}$ uses ...
0
votes
0answers
9 views

Trends in Single Bond Enthalpy of All Nonmetal Groups

Here I have a list of single bond enthalpies, $\ce{X-X}$, in kJ/mol, for the nonmetals arranged by group: Group 7: F: 155 Cl: 242 Br: 193 I: 151 Group 6: O: 146 S: 266 Se: 172 Te: 126 ...
1
vote
0answers
35 views

Why is the melting point of magnesium anomalous? [duplicate]

The melting and boiling points for the Group II elements are as follows: $$\begin{array}{ccc} \text{Element} & \text{Melting point / }\mathrm{^\circ C} \\ \hline \ce{Be} & 1289 \\ \ce{Mg} ...
0
votes
1answer
77 views

Bond Type of Lead: Metallic or Network Covalent?

I know that lead is classified as a metal, from its appearance, nonexistent band gap, and its position on the periodic table... etc. However, all of the elements above it (carbon, silicon, germanium, ...
0
votes
0answers
38 views

How does increasing the molecular mass of compounds of homologous series affect solubility?

First of all, I know that increasing the molecular mass decreases the solubility of that compound wrt, of another compound of the homologous series in organic chemistry. My question is how? My text ...
0
votes
1answer
27 views

2nd Electron Affinity of halogens

I have seen questions regarding EA but they were all about the 1st EA so this question is not duplicate. I came across a statement which goes like "2nd EA of halogens is almost zero". How is this ...
0
votes
1answer
40 views

What is the correct order of chemical reactivity in terms of oxidising property for the following elements: F, Cl, O, and N

This is a textbook question. I am confused as to which factors i should consider while sorting out these elements. If I take electron gain enthalpy, then Cl should be greater than F, but if i consider ...
1
vote
0answers
8 views

Melting temperature and electronegativity trends in transition metals [duplicate]

So I know that generally the melting temperature increases across the row (let's look at just the first row for now) but what are the deviations? And why do they occur? I've looked everywhere online ...
0
votes
0answers
11 views

Reverse trend in solubilty for alkali metals

In case of alkali metals, why does ENTHALPY OF FORMATION for fluorides become less negative down the group and opposite for chlorides, bromides and iodides ?
3
votes
0answers
25 views

Trends in the covalency of bonding across the transition metals

I am under the impression that the covalent character in the bonding of transition metal compounds increases across a group; in fact I think this is why they're called transition metals (a transition ...
5
votes
1answer
49 views

Deviation of Ytterbium from general trend

What is the reason for deviation of ytterbium from the general trend of lanthanides in terms of hardness, melting point, density etc.?
4
votes
2answers
167 views

Why ground-state configuration is consistent (“additive”) from one element to the next?

Ground-state configuration ("electron shells") is consistent throughout the periodic table, for example: (source) Why is it this way if the Hamiltonian of each atom is different? In other words, why ...
1
vote
0answers
35 views

Why is Iron (Fe) difficult to reduce?

$\ce{Fe^3+ + e- -> Fe^2+} \quad +0.77$ $\ce{Fe^3+ + 3e- -> Fe} \quad -0.04$ $\ce{Fe^2+ + 2e- -> Fe} \quad -0.41$ $\ce{Zn^2+ + 2e- -> Zn} \quad -0.76$ $\ce{Co^2+ + 2e- -> Co} \quad ...
2
votes
5answers
450 views

In the periodic table, why doesn't the 2nd row have exactly 2 elements?

Row 1: 2 elements Row 2: 8 elements Row 3: 8 elements Row 4: 18 elements Row 5: 18 elements Row 6: 32 elements Row 7: 32 elements In other words: 2, 8, 8, 18, 18, 32, 32 Why does the first ...
0
votes
0answers
32 views

Difference in the change in oxidation states of transition elements and p-block elements

In transition elements the oxidation states differ by one (+2 to +7 in Mn). However, in the p-block elements, the oxidation states differ by two (-1,+1,+3,+5 in the halogen group). Why is this so?
5
votes
0answers
70 views

Increasing Covalent character increases Colour intensity

I observed some trends as follows:- $\ce{PbCl2}$ white and $\ce{PbI2}$ yellow $\ce{SnCl2}$ white, $\ce{SnCl4}$ red and $\ce{SnI4}$ black $\ce{AgCl}$ white, $\ce{AgI}$, $\ce{AgBr}$ and ...
1
vote
1answer
70 views

Why is the periodic table periodic?

I am not a chemist, but I am interested in Science in a general sense. Can anybody explain why the periodic table is periodic in nature? I would appreciate links for further reading.
1
vote
1answer
32 views

Why does ionization increase from Li to Be? [duplicate]

If ionization energy decreases from $\ce{N}$ to $\ce{O}$ due to the pairing of electrons (causing electric repulsion and greater potential energy) in the $\mathrm{2p}$ orbital in the $\ce{O}$ atom, ...
0
votes
2answers
86 views

Why is Aluminum's 2nd ionization energy higher than Silicon's?

According to the periodic table trend for I.E. Silicon should have a higher 2nd ionization energy than Aluminum so I'm confused.
0
votes
1answer
105 views

Why is Mo(VI) more stable than Cr (VI)?

Acids of $\ce{Mo}^\mathrm{VI}$ are more stable than those of $\ce{Cr}^\mathrm{VI}$ in terms of redox reactivity. In p-block elements, as we go down the groups, the stability of lower oxidation state ...
3
votes
1answer
183 views

Why is fluorine more reactive than iodine despite the weaker I-I bond?

The atomic radii of halogen increases as we go down the group due to addition of new shells. As a result, bond length of halogen $\ce{X-X}$ increases down the group. so, less energy is required to ...
1
vote
1answer
243 views

How long the block starting with element 121 will be?

I remember from my chemistry classes that (after the initial irregularities) a new block of elements starts every two periods. After the initial s-block and p-block following it shortly, we have ...
18
votes
1answer
286 views

Why does tin form tin (II) compounds?

The stability of the +II oxidation state in lead has been widely attributed to the so-called “inert pair effect”: the 6s subshell is stabilized through relativistic contraction due to the near-c speed ...
3
votes
1answer
306 views

Why does the boiling and melting point decrease as you go down group 1 and vice versa for group 7?

I used to think that because an alkali metal needs to lose one electron to complete its outer shell, when the atom increases in size (atomic radius), the electron would be easier to lose as the ...
2
votes
1answer
139 views

Why ionic radii of Cu2+ is less than Zn2+?

Fully filled orbital has more effective nuclear charge than incompletely filled orbital. So atomic or ionic radii of elements or ions having fully filled orbitals should be less than that of elements ...
4
votes
2answers
74 views

How to tell which compound has the biggest ionization energy?

I am preparing for my final exam, and I am very confused about ionization energy. An example question would be: Between the species $\ce{Ne, Na+, Mg^2+, Ar, K+, $\&$~Ca^2+}$, which one has the ...
0
votes
0answers
147 views

Electron affinity of Group 15 elements

The electron affinities of elements in the same group should decrease as you go down the group, but in the Group 15 elements the values generally increase: $$\begin{array}{cc} \hline \text{Element} ...
1
vote
0answers
34 views

How does the electron configuration of platinum relate to its stability?

Does platinum's electron configuration, [Xe] 4f14 5d9 6s1, influence its reactivity and stability? Is the electron configuration the primary contributing factor to platinum's relative inertness? ...
1
vote
0answers
98 views

Why is ionisation energy of bismuth lower than lead?

Why is ionisation enthalpy of Bismuth less than that of Lead for it just comes after the latter in periodic table? First ionisation energy of bismuth is 703 kg/mol while that of lead is 715 kg/mol. I ...
0
votes
1answer
222 views

Why do the melting points of Group 15 elements increase upto Arsenic but then decrease upto Bismuth?

The boiling points of group 15 elements increase on going down the group (or, as size increases) but the same is not true for the melting points. The melting points increase from $\ce{N}$ to $\ce{As}$ ...
2
votes
0answers
158 views

What is an 'acidic' oxide?

My book says that: Oxides in higher oxidation states of elements of group 14 are generally more acidic than those in lower oxidation states.The dioxides $\ce{CO2}$, $\ce{SiO2}$ and $\ce{GeO2}$ are ...
3
votes
1answer
60 views

Periodic table- quantum numbers

I have come across many questions like: "if electron had 3 spins (-1/2,0,+12) then what change will be there in the periodic table?", also sometimes " if the capacity of each orbital becomes 5 then in ...
1
vote
1answer
114 views

Ionization energy and Electron Affnity

Which of the following statements correctly interprets the relationship between ionization energy, atomic radius Electron affinity when comparing two atoms. The correct choice as per my instructor ...
2
votes
1answer
187 views

What is the lattice structure of manganese?

A transition element is defined as the one which has incompletely filled d orbital in its ground state or in any one of its oxidation state. Zinc , cadmium and mercury are not typical transition ...
1
vote
1answer
692 views

Memorizing polyatomic ions? Using Periodic Table

In my Chemistry course, we must memorize a list of common polyatomic ions. Is their an easy way of memorizing ions such as Sulfate $\ce{SO4^2-}$ by looking at just the periodic table. I listed the ...
10
votes
1answer
185 views

Is it possible that atoms with 120 protons are possible, but that atoms with 119 protons aren't possible?

We currently know that there are atoms with atomic number up to 118 are possible. Is it possible that atoms with 120 protons are possible, but that atoms with 119 protons aren't possible? Or are ...
2
votes
3answers
2k views

Why does electronegativity increase as effective nuclear charge increases?

I know that electronegativity is the ability to attract shared electrons and that effective nuclear charge is the pull of the nucleus on outer electrons based on my notes. But I'm not really sure ...
0
votes
0answers
66 views

Why can't element with paired electron have colour

I know that element with unpaired electrons give out colour especially the d-block element which can be explained by crystal field theory. But, why can't element with paired electrons give colour, is ...
1
vote
0answers
265 views

Anomalous behavior of 1st member of s and p block

Why do the first member of each group of s and p-block elements show anomalous behavior? Is it because of their small size or high electronegativity ??