Name: acid and base strength in water
Uploaded: 2025-10-30T13:58:47.000Z
Duration: 3 min 2 s
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NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.5

acidbase-strengths-and-dissociation-constants

Acid/Base Strengths and Dissociation Constants

Asitler ve bazlar, güçlü bir asit, güçlü bir baz, zayıf bir asit veya zayıf bir baz olup olmadıklarına göre kategorize edilebilir. Çok az kuvvetli asit ve baz vardır, bu nedenle asitlerin ve bazların çoğu zayıftır. Hidroklorik asit gibi güçlü bir asit, suda çözündüğünde hidrojen iyonlarına ve klorür iyonlarına tamamen ayrışır.Sodyum hidroksit gibi güçlü bir baz, sodyum iyonlarına ve hidroksit iyonlarına ayrışır. Zayıf asitler ve bazlar kısmen ayrışır ve hem iyonize hem de iyonize olmayan formlarda bulunur. Örneğin, hem asetik asit hem de onun zayıf eşlenik bazı asetat, sulu bir çözelti içinde bulunur.Zayıf bir asit veya bazın ayrışma derecesi, denge sabiti kullanılarak ölçülebilir. Zayıf asitler için denge sabitinin özel bir adı vardır, asit ayrışma sabiti veya Ka.Genel bir zayıf asit HA için, belirli bir sıcaklıktaki Ka değeri bir denge denklemi ile hesaplanabilir:ürünlerin yani A ve hidronyum iyon konsantrasyonlarının reaktanlar yani HA ve su konsantrasyonu ile bölümü. Su sıvı olduğundan ve konsantrasyonu reaksiyonda neredeyse değişmeden kaldığından, denklemden çıkarılır.Ka ne kadar yüksekse asit o kadar güçlüdür. Nitröz asit, asetik asitten daha güçlüdür çünkü nitröz asidin Ka'sı, asetik asidin Ka'sından daha büyüktür. Zayıf bazlar için denge sabiti, baz ayrışma sabiti veya Kb, Ka'ya benzer şekilde hareket eder.Genel bir zayıf baz B için, belirli bir sıcaklıktaki Kb, ürünlerin, BH iyonunun ve hidroksit iyonunun konsantrasyonunun, reaktan B'nin konsantrasyonuna bölünmesiyle belirlenebilir. Asitler gibi, bazların gücü de Kb ile doğru orantılıdır. Örneğin, etilamin üreden nispeten daha güçlüdür çünkü etilamin Kb'si ürenin Kb'sinden daha büyüktür.Bir asidin kuvveti, iyonlaşma yüzdesi olarak da ifade edilebilir. Asidin iyonlaşma yüzdesi, dengede hidronyum iyon konsantrasyonunun ilk asit konsantrasyonuna bölünmesi ve yüz ile çarpılmasıyla hesaplanabilir. Benzer şekilde, bazlar için iyonlaşma yüzdesi dengede hidroksit iyonu konsantrasyonunun başlangıçtaki baz konsantrasyonuna bölünmesi ve yüz ile çarpılmasıyla hesaplanabilir.İyonlaşma yüzdesi ne kadar yüksekse asit veya baz o kadar güçlüdür.

asit/baz güçleri ve ayrışma sabitleri

Bir asidin veya bazın göreceli gücü, suda çözündüğünde ne kadar iyonize olduğu ile ilişkilidir. İyonizasyon reaksiyonu esas itibarıyla tamamlanırsa, asit veya baz güçlü olarak adlandırılır; nispeten az iyonlaşma meydana gelirse, asit veya baz zayıftır. Güçlü olanlardan çok daha fazla zayıf asit ve baz vardır. En yaygın güçlü asitler ve bazlar aşağıda listelenmiştir:
 <table style=""margin-left: auto; margin-right: auto;"">
 <tbody>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Güçlü Asitler</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Güçlü Bazlar</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HClO4</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">LiOH</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HCl</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">NaOH</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HBr</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">KOH</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HI</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Ca(OH)2</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HNO3</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Sr(OH)2</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">H2SO4</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Ba(OH)2</td>
 </tr>
 </tbody>
 </table>
 
 Asitlerin göreli kuvvetleri, sulu çözeltilerde denge sabitleri ölçülerek belirlenebilir. Aynı konsantrasyondaki çözeltilerde, daha güçlü asitler daha büyük ölçüde iyonize olur ve bu nedenle, zayıf asitlerden daha yüksek konsantrasyonlarda hidronyum iyonları verir. Bir asit için denge sabiti, asit iyonizasyon sabiti Ka olarak adlandırılır. Bir asidin reaksiyonu için HA:   
 
 <img alt=""Eq1"" src=""/files/ftp_upload/11395/11395eq1.png"" style=""text-align: center; height: 50px;"" />
 
 Asit iyonizasyon sabiti,   olarak yazılır
 
 <img alt=""Eq2"" src=""/files/ftp_upload/11395/11395eq2.png"" style=""text-align: center; height: 90px;"" />
 
 burada konsantrasyonlar dengede olanlardır. Su reaksiyonda bir reaktan olmasına rağmen, aynı zamanda çözücüdür, bu nedenle denklemde [H2O] 'yu dahil etmiyoruz. Bir asidin Ka’sı ne kadar büyükse, H3O+ ve A−’nın bir denge karışımındaki iyonize olmayan asit (HA) konsantrasyonuna göre konsantrasyonları o kadar büyüktür ve o kadar güçlü asittir. Bir asit, tam iyonizasyona uğradığında “güçlü” olarak sınıflandırılır; bu durumda HA konsantrasyonu sıfırdır ve asit iyonizasyon sabiti ölçülemeyecek kadar büyüktür (Ka≈ ∞). Kısmen iyonize olan asitler “zayıf” olarak adlandırılır ve asit iyonlaşma sabitleri deneysel olarak ölçülebilir.
 
 Bu fikri açıklamak için, aşağıda üç asit iyonizasyon denklemi ve Ka değeri gösterilmektedir. İyonizasyon sabitleri listelenen denklemlerin ilkinden sonuncusuna doğru artar, bu da CH3CO2H < HNO2 < HSO4− sırasındaki nispi asit kuvvetindeki artışları gösterir. 
 
 <img alt=""Eq3-5"" src=""/files/ftp_upload/11395/11395eq3-5.png"" style=""text-align: center; height: 135px;"" />
 
 Bir asidin kuvvetinin bir başka ölçüsü de iyonlaşma yüzdesidir. Zayıf bir asidin iyonlaşma yüzdesi, bir denge karışımının bileşimi cinsinden tanımlanır: 
 
 <img alt=""Eq6"" src=""/files/ftp_upload/11395/11395eq6.png"" style=""text-align: center; height: 90px;"" />
 
 Burada numaratör, asidin eşlenik bazının konsantrasyonuna eşdeğerdir (stokiyometri başına, [A−] = [H3O+]). Ka değerinden farklı olarak, zayıf bir asidin iyonlaşma yüzdesi, başlangıçtaki asit konsantrasyonuna göre değişir ve genellikle konsantrasyon arttıkça azalır.
 
 Tıpkı asitler için olduğu gibi, bir bazın göreli kuvveti, sulu çözeltilerdeki baz iyonlaşma sabitinin (Kb) büyüklüğünde yansıtılır. Aynı konsantrasyondaki çözeltilerde, daha güçlü bazlar daha büyük ölçüde iyonize olur ve bu nedenle, zayıf bazlardan daha yüksek hidroksit iyon konsantrasyonları verir. Daha güçlü bir baz, zayıf bir baza göre daha büyük bir iyonizasyon sabitine sahiptir. Bir bazın reaksiyonu için, B: 
 
 <img alt=""Eq7"" src=""/files/ftp_upload/11395/11395eq7.png"" style=""text-align: center; height: 50px;"" />
 
 İyonlaşma sabiti   olarak yazılır.
 
 <img alt=""Eq8"" src=""/files/ftp_upload/11395/11395eq8.png"" style=""text-align: center; height: 90px;"" />
 
 Aşağıda sunulan üç zayıf baz için verilerin incelenmesi, NO2− < CH2 CO2− < NH3 sırasındaki temel kuvvet artışlarını göstermektedir.
 
 <img alt=""Eq9-11"" src=""/files/ftp_upload/11395/11395eq9-11.png"" style=""text-align: center; height: 135px;"" />
 
 Asitlere gelince, bir bazın göreceli kuvveti aynı zamanda iyonlaşma yüzdesine de yansıtılır
 
 <img alt=""Eq12"" src=""/files/ftp_upload/11395/11395eq12.png"" style=""text-align: center; height: 90px;"" />
 
 Ancak baz iyonizasyon sabitine ve çözeltinin başlangıç konsantrasyonuna bağlı olarak değişecektir.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"">Openstax, Chemistry 2e, Section 14.3: Relative Strengths of Acids and Bases.</a>

Asit/Baz Güçleri ve Ayrışma Sabitleri

Bir asit veya bazın nispi kuvveti, suda çözündüğünde iyonlaşma derecesidir. İyonlaşma reaksiyonu esasen tamamlanmışsa, ...

Education

JoVE Core

Chemistry

Kimya

Acids and Bases

Asitler ve Bazlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

acid and base strength in water

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones.

The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water.

Acid strength can be measured with the acid-ionization constant, Ka. For an acid HA in water, Ka compares the concentrations of the products and the nonionized acid at equilibrium. Water is a reactant in the reaction, but it is not included in the equation because it is the solvent. A larger Ka means more H3O+ and A− relative to HA, so the acid is stronger.

A strong acid is considered completely ionized. In that case, the concentration of HA is zero, and Ka is immeasurably large, or approximately infinite. Weak acids ionize only partially, so their Ka values can be measured in the lab. The relative acid strengths in the examples increase in the order CH3CO2H &lt; HNO2 &lt; HSO4−.

Percent ionization is another way to describe weak acid strength. It is based on the amount of acid that ionizes at equilibrium. For a weak acid, the percent ionization changes with the starting concentration and usually gets smaller as the concentration gets higher. This makes percent ionization different from Ka.

Base strength is measured in a similar way with the base-ionization constant, Kb. For a base B in water, a larger Kb means the base ionizes more and produces a higher hydroxide ion concentration. A stronger base has a larger ionization constant than a weaker base.

The examples of weak bases show the strength order NO2− &lt; CH2CO2− &lt; NH3. Base strength can also be described with percent ionization. As with weak acids, this value depends on both the base-ionization constant and the initial concentration of the solution.

Acid and Base Strength in Water

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

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

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...

ions as acids and bases

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

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

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

acid strength and molecular structure

How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how acid and base strength in water depends on ionization, Ka, Kb, and percent ionization, with examples of strong and weak acids and bases.

Acid and Base Strength in Water | JoVE K12

chemistry

JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

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9-12.C.1.6.c

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New York State Science Learning Standards

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Georgia Standards of Excellence

SPS6.

Acid and Base Structure

SC6.

acids-and-bases-percent-dissociation-and-ph

Acids and Bases: Percent Dissociation and pH

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

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Colloids

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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 ...

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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

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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 ...

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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 ...

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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 ...

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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

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atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

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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

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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

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Halogens

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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 ...

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.

Acid and Base Strength in Water

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