Name: salt hydrolysis and ph in solutions
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 4 min 8 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.5

Determining the pH of Salt Solutions

염용액은 산성, 염기성 또는 중성일 수 있습니다. 개별 이온들을 검사하여 용액의 pH가 7 이하인지, 이상인지 또는 같은 지를 확인할 수 있습니다. pH 중성 양이온 및 음이온이 함유된 염은 중성 용액을 생성합니다.

이 염은 강산과 강염기의 상대이온으로 구성되어 있습니다. 순수한 질산칼륨 수용액은 칼륨과 질산염 모두 산성 또는 염기성 성질을 가지고 있지 않기 때문에 pH가 7일것입니다. 약염기의 상대이온인 양이온과 강산의 상대이온인 음이온이 포함된 염은 pH가 7보다 작습니다.

브롬화 암모늄 용액에서 브롬화 이온은 pH가 중성인 반면 암모늄 이온은 산성이며 물 분자에 양성자를 기증합니다. 강염기의 대상이온인 양이온과 약산의 대상이온인 음이온이 포함된 염은 pH가 7보다 큽니다. 아세트산 나트륨 용액에서 나트륨 이온은 pH가 중성인 반면 아세테이트 이온은 염기성이고 물 분자로부터 양성자를 받아들입니다.

일부 염에는 각각 약산과 약염기의 대상이온인 양이온과 음이온이 들어 있습니다. 용액은 양이온의 Ka가 음이온의 Kb보다 크면 산성이고 음이온의 Kb가 양이온의 Ka보다 크면 염기성이며 Ka와 Kb가 같으면 중성입니다. 아질산암모늄 용액에서 암모늄의 Ka는 아질산 이온의 Kb보다 크기 때문에 산성이 됩니다.

산성 또는 염기성 이온을 포함하는 염 용액의 정확한 pH는 해당 이온의 짝산 또는 짝염기에 대한 해리 상수를 사용하여 결정할 수 있습니다. 0.35M 시안화 나트륨의 pH는 짝산인 시안화 수소산의 Ka에서 시안화물의 kb를 계산하고 ICE 표를 설정하여 평형 농도를 결정함으로써 계산할 수 있습니다. 나트륨 양이온은 물과 반응하지 않으므로 pH에 영향을 주지 않으며 따라서 무시할 수 있습니다.

이와 대조적으로 시안화 이온은 물 분자로부터 양자를 받아들여 수산화 이온을 생성합니다. 시안화 이온의 Kb는 Ka x Kb Kw라는 방정식을 사용하여 결정할 수 있습니다. 시안화 수소산의 Ka는 4.90 10⁻¹⁰이므로 시안화 이온의 Kb는 2.04 10⁻⁵입니다.

Kb는 시안화 수소산 농도와 수산화물 이온 농도를 곱하고 시안화 이온의 농도로 나눈 값과 같습니다. ICE 표를 구성하여 초기 농도 및 평형 농도를 표현할 수 있습니다. 평형 농도 값을 식에 대입하면 Kb는 x 곱하기 x를 0.35로 나눈 값으로 나중에 5 퍼센트 규칙으로 확인할 수 있습니다.

방정식을 풀면 x는 2.7 10⁻³ 몰과 같습니다. x는 0.35M의 0.77 퍼센트에 불과하므로 근사치 0.35 빼기 x는 0.35와 같습니다. 용액의 pOH는 2.7 10⁻³ 몰의 음의 로그를 취하여 계산할 수 있으며 값은 2.57입니다.

용액의 pH는 방정식 pH pOH 14을 사용하여 결정할 수 있으며 따라서 이 시안화 나트륨 용액의 pH는 11.43입니다.

염 용액의 ph 결정

염 용액의 pH는 음이온과 양이온 성분에 의해 결정됩니다. pH 중성 음이온과 하이드로늄 이온 생성 양이온을 포함하는 염은 pH 7 미만의 용액을 형성합니다. 예를 들어 질산암모늄(NH_4NO^3) 용액에서 NO_3^- 이온은 물과 반응하지 않는 반면 NH_4^+ 이온은 하이드로늄 이온을 생성합니다. 결과적으로 산성 용액이 생성됩니다. 대조적으로, pH 중성 양이온과 수산화물 이온 생성 음이온을 포함하는 염은 pH가 7보다 큰 용액을 형성합니다. 예를 들어 불화나트륨(NaF) 용액에서 Na^+는 pH 중성이지만 F^-는 다음을 생성합니다. 수산화물 이온을 생성하여 염기성 용액을 형성합니다. 강산 또는 강염기의 반대 이온은 pH 중성이며 이러한 반대 이온에 의해 형성된 염은 pH가 7인 중성 용액을 형성합니다. 예를 들어 KBr에서 K^+ 양이온은 불활성이며 pH에 영향을 미치지 않습니다. 브롬화물 이온은 강산의 짝염기이므로 염기 강도는 무시할 수 있습니다(염기 이온화는 감지할 수 없음). 용액은 중성입니다.

일부 염에는 산성 양이온과 염기성 음이온이 모두 포함되어 있습니다. 용액의 전반적인 산도 또는 염기도는 양이온과 음이온의 상대적 강도에 의해 결정되며, 이는 K_a와 K_b를 사용하여 비교할 수 있습니다. 예를 들어, NH_4F에서 NH_4^+ 이온은 산성이고 F^- 이온은 염기성(약산성 HF의 공액염기)입니다. 두 이온화 상수를 비교하면 NH_4^+의 K_a는 5.6 × 10^−10이고 F−의 K_b는 1.6 × 10^−11이므로 K_a > K_b이므로 용액은 산성입니다.

산성 염 용액의 pH 계산

아닐린은 염료 제조에 사용되는 아민입니다. 이는 약염기 아닐린과 염산의 반응으로 제조된 염인 염화아닐리늄([C_6H_5NH_3^+]Cl)으로 분리됩니다. 0.233M 염화아닐리늄 용액의 pH는 얼마일까요?

<img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />

아닐리늄 이온의 K_a는 짝염기인 아닐린의 K_b에서 파생됩니다.

<img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />

제공된 정보를 사용하여 이 시스템에 대한 ICE 테이블이 준비됩니다.

<div class="overflow">
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"></td>
			<td style="color: black; border: 1px solid black; text-align: center;">C6H5NH3+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">C6H5NH2 (aq)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">초기 농도(M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.233</td>
			<td style="color: black; border: 1px solid black; text-align: center;">~0</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">변경(M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">-x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">평형 농도 (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.233 - x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ⅹ</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ⅹ</td>
		</tr>
	</tbody>
</table>
</div>

이러한 평형 농도 항을 K_a 식으로 대체하면 다음과 같습니다.

<img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />

x << 0.233이라고 가정하면 방정식이 단순화되어 x에 대해 해결됩니다.

<img alt="Eq4" src="/files/ftp_upload/11404/11404_Equation_4.png" style="height: 90px;" />

<img alt="Eq5" src="/files/ftp_upload/11404/11404_Equation_5.png" style="height: 50px;" />

ICE 테이블은 x를 하이드로늄 이온 몰농도로 정의하므로 pH는 다음과 같이 계산됩니다.

<img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />

[Al(H_2O)_6]^3+의 가수분해

완전히 용해되어 용액에 수화된 알루미늄 이온 [Al(H_2O)_6]^3+이 생성되는 0.10M 염화알루미늄 용액의 pH를 계산해 보세요.

반응식과 K_a는 다음과 같습니다.

<img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />

제공된 정보가 포함된 ICE 테이블은 다음과 같습니다.

<div class="overflow">
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"></td>
			<td style="color: black; border: 1px solid black; text-align: center;">알(H2O)63+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">알(H2O)5(OH)2+ (aq)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">초기 농도(M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.10</td>
			<td style="color: black; border: 1px solid black; text-align: center;">~0</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">변경(M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">-x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">평형 농도 (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.10 - x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ⅹ</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ⅹ</td>
		</tr>
	</tbody>
</table>
</div>

평형 농도에 대한 식을 이온화 상수에 대한 방정식으로 대체하면 다음과 같은 결과가 나옵니다.

<img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />

x << 0.10이라고 가정하고 단순화된 방정식을 풀면 다음이 제공됩니다.

<img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />

ICE 표에서는 x를 하이드로늄 이온 농도와 동일하게 정의하므로 pH는 2.92로 계산되며 용액은 산성입니다.

<img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />

이 문서는 에서 발췌되었습니다  <a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>.

염 용액의 pH 결정

염 용액의 pH는 구성 요소 음이온과 양이온에 의해 결정됩니다. pH 중성 음이온과 히드로늄 이온 생성 양이온을 포함하는 염 ...

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salt hydrolysis and ph in solutions

Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral.

Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic.

Other salts contain pH-neutral cations and anions that produce hydroxide ions. These salts form basic solutions with pH above 7. Sodium fluoride is an example. In NaF, Na+ is pH-neutral, while F− reacts with water to produce hydroxide ions.

Salts made from the counterions of a strong acid or a strong base are usually neutral. Their solutions have a pH of 7. In KBr, K+ is inert and does not change the pH. Br− is the conjugate base of a strong acid, so it has negligible base strength and does not appreciably ionize in water.

Some salts contain both an acidic cation and a basic anion. In those cases, the overall pH depends on which ion is stronger. The ionization constants Ka and Kb are used to compare them. For NH4F, NH4+ is acidic and F− is basic. Because Ka for NH4+ is 5.6 × 10−10 and Kb for F− is 1.6 × 10−11, the solution is acidic since Ka is greater than Kb.

The pH of an acidic salt solution can be calculated with an ICE table. Anilinium chloride, [C6H5NH3+]Cl, comes from the weak base aniline and hydrochloric acid. For a 0.233 M solution, the Ka value for the anilinium ion is found from the Kb of aniline. The ICE table gives x as the hydronium ion concentration, and the pH is then calculated from that value.

Hydrolysis of the hydrated aluminum ion works the same way. Aluminum chloride dissolves completely to give [Al(H2O)6]3+ in solution. For a 0.10 M solution, the reaction and Ka are set up in an ICE table. After assuming x is much smaller than 0.10 and solving the simplified equation, the hydronium ion concentration gives a pH of 2.92. The solution is acidic.

Salt Hydrolysis and pH in Solutions

bronsted-lowry acids and bases

Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

water: a bronsted-lowry acid and base

Water as an Amphiprotic Substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

ph scale

pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

relative strengths of conjugate acid-base pairs

relative-strengths-of-conjugate-acid-base-pairs

How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong Acids, Strong Bases, and pH

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weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

weak base solutions

Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

mixtures of acids

pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

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Salt Hydrolysis and pH of Solutions

Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

determining the ph of salt solutions

Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

acidbase-strengths-and-dissociation-constants

Acid and Base Strength in Water

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How Bonding Affects Acid Strength

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Electron-Pair Reactions in Acid-Base Chemistry

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key terms and concepts

Learn how salt ions affect pH, from acidic ammonium salts and basic fluoride salts to neutral salts and pH calculations with ICE tables.

Salt Hydrolysis and pH in Solutions | JoVE K12

chemistry

JoVE Core 화학은 간결하고 이해하기 쉬운 애니메이션을 통해 일반 화학 개념을 설명합니다. 또한, 과학자가 직접 고전실험과 연구실험을 진행하는 실사 영상을 제공합니다.

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Texas Essential Knowledge and Skills

High School

CHEM.12

CHEM.12.D

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6

9-12.C.1.6.d

9-12.PS.3.6.c

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Molecules and Compounds

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Colloids

Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera ...

Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

phase-transitions-vaporization-and-condensation

Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

phase-transitions-sublimation-and-deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

PS.PSc.1.5

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

IUPAC Nomenclature of Ketones

Like aldehydes, ketones are named using IUPAC rules; in this case, by replacing &#8220;e&#8221; in the name of the longest hydrocarbon chain with ...

IUPAC Nomenclature of Carboxylic Acids

IUPAC names of carboxylic acids are systematically derived following a few rules discussed below.
For acyclic saturated monocarboxylic acids, the longest ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Salt Hydrolysis and pH in Solutions

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