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4 years ago

If two nonmetals with the same electronegativity bond, what type of bond will form?

2 answers:

7 0

If two nonmetals with the same electronegativity bond, what type of bond will form then Non polar covalent bond (option D) will form.

AlladinOne [14]4 years ago

6 0

Answer:

Two nonmetals with the same electronegativity will form a non polar covalent bond.

Explanation:

The type of bond between atoms is classified in 3 big groups:

Metallic bond: this type of bond only take place between metallic atoms like Cu, Al, Au, etc.

Ionic bond: this type of bond is formed between ions, that means that it is necessary the presence of a cation (ion with positive charge) and and an anion (ion with negative charge) and when the atoms has a very high difference of electronegativity (more that 2), that makes the ionic bond always polar, because there will be always a positive pole (cation) and a negative pole (anion). This is common between a metal and a nonmetal, for example: sodium chloride (NaCl).
Covalent bond: this type of bond occurs when atoms share one or more pairs of electrons, this happens between nonmetals, e.g.: the molecule of chlorine gas (Cl₂).

Apart from that, depending on the electronegativity difference, the covalent bonds are clasified in polar and non polar:

- Polar covalent bond: the difference of electronegativity is important but less than an ionic bond (between 0 and 2).

- Non polar covalent bond: this occurs when the atoms forming bonds have the same electronegativity.

So, analyzing the statement, if we have two nonmetals it is a covalent bond, and if the two nonmetals atoms have the same electronegativity the bond will be non polar.

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Among K, Ca and Ba, which element possess low ionization energy?

deff fn [24]

Among the elements Barium has the lowest Ionization Energy.

<h3>What is Ionization Process ?</h3>

The process by which any neutral atom gets converted into electrically charged by gaining or losing electron is called Ionization Process.

K is an alkali metal it has to lose one electron to attain stable electronic configuration of an inert gas

For removing second electron , a stable configuration has to be broken and so will require high amount of energy.

Ca and Ba are alkaline earth metals.

They both have to lose 2 electrons to attain stable electronic configuration of noble gas.

They have low Iow Ionization Energy as compared to K.

Ca has higher Ionization Energy as compared to Ba because when we move down the periodic table , The ionization energy decreases.

Hence , Among the elements Barium has the lowest Ionization Energy.

To know more about Ionization Process

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5 0

2 years ago

How many molecules are there in 46.0 g of ethanol, CH 3 CH 2OH?

lilavasa [31]

Answer:

Explanation:

6 0

3 years ago

How are you guys Now help me

KengaRu [80]

Answer:

Explanation:

im sorry dont knwo

i think its the second one

6 0

3 years ago

How many molecules are in a 189 g sample of carbon tetrabromide, CBr4 ?

anyanavicka [17]

Answer:

3.4 × 10²³ molecules of CBr₄

Explanation:

Given data:

Mass of CBr₄ = 189 g

Number of molecules = ?

Solution:

First of all we will calculate the number of moles.

Number of moles = mass / molar mass

Number of moles = 189 g/ 331.63 g/mol

Number of moles = 0.6 mol

Now the given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

Foe 0.6 moles of CBr₄:

0.6 mol × 6.022 × 10²³ molecules of CBr₄ / 1 mol

3.4 × 10²³ molecules of CBr₄

5 0

3 years ago

Sodium symbol and charge, and use this to determine the compounds formula?

Leni [432]

Symbol          Name                    Symbol          Name

H+              hydrogen ion            H-              hydride

Li+             lithium ion             F-             fluoride

Na+             sodium ion              Cl-             chloride

K+              potassium ion           Br-             bromide

Rb+             rubidium ion            I-              iodide

Cs+             cesiumion              O2-              oxide

Be2+             beryllium ion           S2-              sulfide

Mg2+             magnesium ion           Se2-             selenide

Ca2+             calcium ion             Te2-             telluride

Sr2+             strontium ion           N3-              nitride

Ba2+             barium ion              P3-              phosphide

Ra2+             radium ion              As3-             arsenide

Ag+             silver ion

Zn2+             zinc ion                Al3+             aluminum ion

Note that the letters in an ion's name before the -ideending is the stem.

For example, the stem for bromide is brom-. Also, just in case, the P for

phosphide is a capital P.

Symbols and Charges for Monoatomic Ions

Variable Charge

        Systematic nameCommon                  Systematic name Common

Symbol  (Stock system)  name            Symbol  (Stock system)  name

Cu+     copper(I)       cuprous         Hg22+    mercury(I)      mercurous

Cu2+     copper(II)      cupric          Hg2+     mercury(II)     mercuric

Fe2+     iron(II)        ferrous         Pb2+     lead(II)        plumbous

Fe3+     iron(III)       ferric          Pb4+     lead(IV)        plumbic

Sn2+     tin(II)         stannous        Co2+     cobalt(II)      cobaltous

Sn4+     tin(IV)         stannic         Co3+     cobalt(III)     cobaltic

Cr2+     chromium(II)    chromous        Ni2+     nickel(II)      nickelous

Cr3+     chromium(III)   chromic         Ni4+     nickel(IV)      nickelic

Mn2+     manganese(II)   manganous       Au+     gold(I)         aurous

Mn3+     manganese(III)  manganic        Au3+     gold(III)       auric

Symbols and Charges for Polyatomic Ions

Formula         Name                    Formula         Name

NO3-             nitrate                 ClO4-            perchlorate

NO2-             nitrite                 ClO3-            chlorate

CrO42-           chromate                ClO2-            chlorite

Cr2O72-           dichromate              ClO-            hypochlorite

CN-             cyanide                 IO4-             periodate

MnO4-            permanganate            IO3-             iodate

OH-             hydroxide               IO-            hypoiodite

O22-             peroxide                BrO3-            bromate

NH2-             amide                   BrO-            hypobromite

CO32-            carbonate               HCO3-            hydrogen carbonate (bicarbonate)

SO42-            sulfate                 HSO4-            hydrogen sulfate (bisulfate)

SO32-            sulfite                 HSO3-            hydrogen sulfite (bisulfite)

C2O42-            oxalate                 HC2O4-           hydrogenoxalate (binoxalate)

PO43-            phosphate               HPO42-           hydrogen phosphate

PO33-            phosphite               H2PO4-           dihydrogen phosphate

S2O32-            thiosulfate             HS-             hydrogen sulfide

AsO43-           arsenate                BO33-            borate

SeO42-           selenate                B4O72-            tetraborate

SiO32-           silicate                SiF62-           hexafluorosilicate

C4H4O62-  tartrate

C2H3O2-           acetate  (an alternate way to write acetate is CH3COO-)

There is one positive polyatomic ion. It is NH4+and is called the ammonium ion.

Note: Writing just the plus sign or minus sign for ions with +1 or -1 charges is

acceptable.

Binary Compounds of Metals with Fixed Charges

Given Formula, Write the Name

A binary compound is one made of two different elements. There can be one of each element such as in NaCl or KF. There can also be several of each element such as Na2O or AlBr3.

Please remember that all elements involved in this lesson have ONLY ONE charge. That includes BOTHthe cation AND the anion involved in the formula.

Points to remember about naming a compound from its formula

1.        The order for names in a binary compound is first the cation, then the anion.

2.        Use the name of cation with a fixed oxidation state directly from the periodic table.

3.        The name of the anion will be made from the root of the element's name plus the suffix "-ide."

Example 1: Write the name of the following formula: H2S

Step #1 - Look at first element and name it. Result of this step = hydrogen.

Step #2 - Look at second element. Use root of its full name ( which is sulf-) plus the ending "-ide." Result of this step = sulfide.

These two steps give the full name of H2S. Notice that the presence of the subscript is ignored. There are other types of binary compounds where you must pay attention to the subscript. Those compounds involve cations with variable charges. Your teacher will tell you which ones you will be held responsible for.

Example 2: Write the name of the following formula: NaCl

Step #1 - Look at first element and name it. Result of this step = sodium.

Step #2 - Look at second element. Use root of its full name ( which is chlor-) plus the ending "-ide." Result of this step = chloride.

Example 3: Write the name of the following formula: MgBr2

Step #1 - Look at first element and name it. Result of this step = magnesium.

Step #2 - Look at second element. Use root of its full name ( which is brom-) plus the ending "-ide." Result of this step = bromide.

Note the presence of the subscript does not play a role in this name.

Example 4: Write the name of the following formula: KCl

The first part of the name comes from the first element symbol: potassium. The second part of the name comes from the root of the second symbol plus '-ide,' therefore chlor + ide = chloride.

This compound is named potassium chloride

Example 5: Write the name of the following formula: Na2S

First symbol is Na, so the first part of the name is sodium. (Note the presence of the subscript does not play a role in this name.) Second element is sulfur (from the symbol S), so the name is sulf + ide = sulfide.

6 0

4 years ago