Chem chapter 5 sec 3

How is the size of an atom defined? How ever this boundary is? And varies under diffrent? Therfor to estimate the size of an atom the conditions that the atom exits in?

Its defined by the edge of its orbital, fuzzy, conditions, must be specified

The elements are ordered in a rough correlation of atomic number and?

Electron configuration

The elements are ordered in the periodic table with their atomic number but their is also another key concept

It depends on the arrangment of electrons in its electron configuration aswell

A way to measure an atoms radius?

Atomic radius

Is to measure the distance between teh nuclei of two identical atoms that are chemially bonded then divide this distance by two

One half teh distance between the nuclei of identical atoms bonded together

The atomic radii decreases gradually from?

The beggining of the Period to the last of the period

In what dimension is it measured in?

Picometers so -12

What does the pictures include?

4 atomic symbole atomic number relative attomic size and atomic radius

trend to smaller atoms accros a period is caused by?

The increasing positeve charge of the nucleus

As electrons add to s and p sublevels in the main energy level , which results in ?

They are gradually pulled closer to the highly chargeed nucleus, a decrease of atomic radius

The energy level is somewhat offset ( tried to be stopped) by? Among who?

The repulsion, among the increased number of electrons in the outer energy level

What happens to the atomic radius when we go down the group? Why?

The atomci radius of what elements increases down a group?

It increases, beacuse electrons ocupy main energy levels farther than the nucleus which causes an increase of the atomic radius

Main group elements

Then why os Al bigger than galium. Which causes galium?

Beacuse galium unlike alaminium is preceded by the d block

The d sublevel does not shield well against the nuclear energy which causes the shrinking of the electron clouds due to the over weighing nuclear charge that is considerably higher than that of Aluminum

How can an electron be removed? Using what as a symbol

It can be removed if enough energy is supplied using, A as a symbol

What does the A+ mean?,what does the single positeev charge mean?

Then what is an ion

Its an ion of an element, 1+ ion

Is an atom or group of bonded atoms that have a negative and positeve charge

Ionzation

To compare the ease with which aoms of diffrent elements give up electrons they compare??

Any procces that results in the formation of an ion is called ionazation

Ionazation energy

What is ionazation energy?

To avoid the influence of near by atoms what do they do?

The energy required to remove an electron of a neutral atom of an element is called ionazation energy

Measurments of ionazation energies are made of isolated atoms in gas phase

In what unit are ionazation energies represenetd in?

Unlike radius they increase and decrease?

Kilo joules/ mole

Accros a period

Accros a group

What group has lowest ionazation energy

Therfore?

Group 1, they lose electrons quite easily ?

If they have low ionazation energy it means?

What is the reason of teh high reactivity of group one?

They lose electrons quite easily

Its beacuse they lose electrons quite easily and make ions

Noble gases ?So? The low reactivity of noble gases is partly based on?

How the highest ionazition energies they dont loss electrons easily, this difficulty of electron removal

Why does the ionazation energy become higher accros a period? A higher charge?So increasing nuclear charge is both responsible?

Beacuse the nuclear energy increases, More strongly attracts electrons in the same energy level

For decrease of atomci radius and increase of ionazation energy

In general do metals or nonmetals have higher ionazation energies ? And for e.x the diffrence between the groups?

Non metals do and for example group 1 does have alot lower ionazation energy requirement than group 18

Only among the main group elements their groups… And why is that? Therfor?And as atomic number increases

These influences overcome

Ionazation energy decrease along the group

Electrons removed from atoms of each element in a group are i higehr energy levels

They are removed more easily

more electrons lie between the nucleas and the electrons highest ocupeid energy levels this shield the outer electrons from the effect of nuclear charge These influences overcome the attraction of the electrons to teh increasing nuclear charge

Teh attraction of the electrons to the increasing nuclear charge

With sufficient energy electrons can be lost from?

What is second ionazation energy?

What is the symbol for ionazation energy? What about second?

Both neutral atoms and positeve ions

The energy needed to remove additional electrons from an atom is reffered

IE IE 2

SO a A+ + energy = A++ + e-

Why? Energy is added when energy is added an eelctron is removed so that makes our element more a positive ion so another symbol will be placed right next to it

Why is the second allways less than the third ionazation and the second is allways higher than the first ionazation?

So each electron removed? So it order to measure it? So basically (. Jjk terms?)

This is beacuse as electrons are removed in succesive ionazations fewer electrons remain within the atom to shield the attractive forces of teh nucleus

From an ion feels increasingly stronger effective nuclear charge its basically teh nuclear charge minus the electron shielding

The nuclear charge - the shielding

It gets hit by a black flash

Removinga n electron from group 18 is more difficult to remove an electron than?This special stability of

any other element in that period

Ions that have noble gas configuration also

Neutral Atoms can also accquire?

Electron affinity And when they acquire an electron they usually? Which makes our a?

Electrons

The energy change that ocures when an electron is acquired by a neatral atom is called the atoms electron affinity

Give off energy ( release ) , negative

The quantity of energy produced is represented

On the other hand some atoms have to be forced to gaina n electron by adding what?

The quantity of energy absrobed Is represented?

What about ions being made this way?

Electron affinity is expressed in?

By a negative number, by adding energy, is represenetd by a positeve number

Ions that are made this way some will be unstable and lose there electron quite easily

Kj per a mol

The ones we have studied are allways measured in?

Numbers

Which group can acquire the electron the most easily? Do they have small or large energy change?

Group 17, they have large, its large its in the negatives

So why is halogens so reactive?

Accros a period the shell number? Group?

Accros a period as electrons are added to the p sub levels of atoms with increasing? What happens?

Explain to me in ur terms

Beacuse they can acquire an electron quite easily and release large amounts of energy

Is constant , its not constant

Nuclear charge, electron affinity becomes more negative charged across each period within the p block

When electrons fill the p sub levels the nuclear chareg increases which brings closer the electron clouds when they do get closer more enrgy is released to get stable so basically the electron affinity increases

An exception of the increase in electron affinity accros a period? Why are they like that?

Between group 14 and 15 carbon and nitrogen

We can half fill the carbon mcuh more easily than to force an electron to nitrogen taht is already half filled

Acros a group?what are the 2 factores? What pre dominates the electron affinity?but there are exceptions to this down a group decreases cuz the size increases

It doesnt specifically have a trend but electrons can be gained by an atom more across a group is more difficult

A slight increase in nuclear energy down a group which that is what increase the affinity

The second is teh increase in the atomic radius down a group which weakens the nuclear charge which makes the electron affinity less

The atomic radius

Espiacially in transition metals some of them stay the same size and some decrease in radius down a group

Its really hard to add an electron to a negative ion therfor? Certain p block nonmetals tend to form? For example which group of elements do by adding an electron?

All second electron affinities are positeve when first made( beacuse they have to absorb energy to start), negative ions that ahve noble ags configuration , the halogens do by adding one electron

For example? Group 16 can aquire stable noble gas configurations by? Nitrogen( group 15), the noble gas configurations for those ones are neons each atom where it becomes stable in the p block it gains the stability of?

Chlorine can get an electron and become a stable electron configuration that has noble gas stability but we cant add another electron only be adding alarge amount of energy

Gettin 2 electrons which becomes a double negative ion

By adding 3 , teh noble gas at the end of the Group

Lanthanids and actinides electron affinity average?

-50 kj per a mol and 0 kj per a mole

A positeve ion is known as? The formation of a cation is by?Causes? Why. Which causes

Cation, lossing one or two electrons causes the atomic radius to decrease, beacuse the removel of teh hightes energy electrons will cause the electron cloud to become smaller, the other electron clouds to be pulled in closer beacuse of teh un even positeve charge

A negative ion is known as? The formation of a anion by? Which allways causes? Why? So the electrons? And the electron cloud also spreads out

Anion, gaining one electron which causes it allways to increase the atomic radius, beacuse the total amount of nuclear energy doesnt change but the electron clouds increases which causes a increase in radius

Were not as strongly pulled in by the nucleus after the electron is added , due to the repulsion between the electron clouds

Within each period the metals and nonmetals

Along a period

Starting from group?

Metals at the left forms cations and the nonmetals at the top right forms anions

The cationic radi ddecreases beacuse the nuclear energy increases and brings the electrons closer to it self

Group 15 beacuse they need 3 electrons to become a stable noble config so basically anions form

Which one are more comon anions or cations? Anions decrease from? Why?

Acros a group?

Anions Group 15 to 18, beacuse of an increase in nuclear energy

Beacuse more furthur electron clouds fill up down a group atomic radius increases so does ionic radii

Chemical compounds are formed Beacuse? The electrons that interact are those in the? Those electrons are the most?

Valence electrons, valence electrons are mostly located in?

Beacuse valence electrons are lost gained or shared between atoms, are the ones located at the outermost energy level

Are the most subjected to nearby atoms or ions , those electrons avialiable to be lost gained or shared in the formation of a chemical compound is known as valence electrons

Incomplete energy levels ( not fileld enrgy levels)

For main group elements the valence electrons are located in? The inner electrons? Held by what? To do what?the group one and two have how many valence electrons? What about group 13-18, in some cases

The outermost s and p sub levels,are in filled energy levels and are held to tightly by the nucleus to do compound formations, Have one ore two elecetrons

They have the amount of valencce electrons by group number minus 10

Reactions from both the s and p levels are involved but in some cases of the group p only p is involved in chemical reactions

Velence electrons hold what together in what?In many compounds the negative charge of the valence electrons

, this un even concentration of charge has a significant, therfor its usefull to know

atoms together in chemical compound, is concentrated to one atom to another, effect on the properties of a compound, to know the measure of how strongly an atom attracts an electron in a compound

Who made a what reflecting the? Where ix he from?

Electronegativity

The most electronegative element is? Its arrbiterally assigned a value of? The values of the otehr elements are?

Linus paulign amde a scale of numerical measurments to measure the tendencu of an atom to attract electrons America

Is the measur4e of teh ability of an atom to attract an electron of another atom in the compound

Flourine, four, determiend by relations to the values of this element

AAccros a period?altough? Which groups are the leats electronegative elements? In makign compounds. What are the most electronegative elements?In compounds?

In increases altghough tehre are exceptions Alkali metals and alkali earth metals, they are the least attracting electrons, its nitogen oxygen and halogens Their atoms attract strongly

Along a group? Noble gases? And when a noble gas does form a compound

They tend to decrease or remain the same

Are unusualy because some of them dont react so they cant be assigned a value

Its electronegartivity is rather high and like that of an halogen

In order where electrons are removed from an atom is in reverse of the order?

Of the elements electron configuration

What are the general trends that are found in groups and periods?

Atomci radius IE electron affinity ionec radii and electronegativity

What is the order of removing electrons from an atom electron configuration?

Its teh opposite of adding atoms to the electron configuration