The correct options are A and B.
The correct ions with noble gas electron configurations are A. [tex]$\mathrm{H}^{-}$[/tex] and B. [tex]$\mathrm{Na}^{+}$[/tex].
The electron configuration of a noble gas is characterized by a completely filled electron shell. Noble gases have electron configurations that end in s²p⁶, where 's' and 'p' represent the electron orbitals. Let's analyze the ions in question:
A. [tex]$\mathrm{H}^{-}$[/tex]: Hydrogen normally has 1 electron in its 1s orbital. However, [tex]$\mathrm{H}^{-}$[/tex] has gained an extra electron, making its electron configuration 1s², which is similar to helium, a noble gas.
B. [tex]$\mathrm{Na}^{+}$[/tex]: Sodium has an electron configuration of [Ne] 3s¹, but [tex]$\mathrm{Na}^{+}$[/tex] loses its 3s¹ electron to become [Ne], which is like a noble gas configuration.
C. [tex]$\mathrm{Br}^{+}$[/tex]: Bromine normally has an electron configuration of [Ar] 3d¹⁰ 4s² 4p⁵. When it loses an electron to form [tex]$\mathrm{Br}^{+}$[/tex], it becomes [Ar] 3d¹⁰ 4s² 4p⁴, which is not a noble gas configuration.
D. [tex]$\mathrm{F}^{+}$[/tex]: Fluorine normally has an electron configuration of [He] 2s² 2p⁵. When it loses an electron to form [tex]$\mathrm{F}^{+}$[/tex], it becomes [He] 2s² 2p⁴, which is not a noble gas configuration.
So, the ions that possess the electron configuration of a noble gas are A. [tex]$\mathrm{H}^{-}$[/tex] and B. [tex]$\mathrm{Na}^{+}$[/tex].
The complete question is here:
Select the ions below which possess the electron configuration of a noble gas.
A. [tex]$\mathrm{H}^{-}$[/tex]
B. [tex]$\mathrm{Na}^{+}$[/tex]
C. [tex]$\mathrm{Br}^{+}$[/tex]
D. [tex]$\mathrm{F}^{+}$[/tex]
The ions Cl-, O2-, H-, and Na+ all have the electron configuration of a noble gas: Cl- matches Argon, O2- matches Neon, H- matches Helium, and Na+ matches Neon.
The question is asking us to identify which ions have the electron configuration of a noble gas. In the periodic table, noble gases have a full outer shell of electrons, typically reaching the stable octet configuration. Let's examine the ions given:
Cl− has an atomic number of 17. In its neutral state, chlorine has the configuration [Ne]3s23p5. Gaining one electron to form Cl− would fill its 3p orbital, achieving the noble gas configuration of [Ar].O2− has an atomic number of 8. In its neutral state, oxygen has the configuration [He]2s22p4. Gaining two electrons to form O2− would fill its 2p orbital, achieving the noble gas configuration of [Ne].H− has an atomic number of 1. In its neutral state, hydrogen has one electron. Gaining one electron to form H− gives it the noble gas configuration of [He].Na+ has an atomic number of 11. In its neutral state, sodium has the configuration [Ne]3s1. Losing one electron to form Na+ would leave it with the noble gas configuration of [Ne].All of these ions indeed match the noble gas configurations; Cl− matches Argon, O2− matches Neon, H− matches Helium, and Na+ matches Neon.
Complete Question: Select the ions below which possess the electron configuration of a noble gas.
Cl−
O2−
H −
Na +
Iki indicator tests for the presence of which substance? benedict's reagent tests for the presence of which substance?
Iki also known as Lugol's solution, is an indicator used to test for the presence of starch. Benedict's reagent is used to test for the presence of reducing sugars, such as glucose and fructose
Lugol's solution is a yellow-brown solution that turns blue-black in the presence of starch.
Benedict's reagent is a clear blue solution that changes color to green, yellow, orange, or red, depending on the amount of reducing sugar present. Benedict's test is commonly used in the laboratory to detect the presence of reducing sugars in various substances.
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Please help! I’m on my last attempt
Write 266000 in scientific notation
which term best describes the rate at which glacial erosion takes place
100 ml of soft drink A contains 75g of sugar and weighs 110g. calculate density
The density of soft drink A is indeed 0.35 g/ml.
Given:
Mass of the soft drink (including sugar) = 110 g
The volume of the soft drink = 100 ml
Mass of sugar = 75 g
First, we need to find the mass of just the liquid (excluding the sugar), then we can calculate the density.
Mass of liquid = Total mass of soft drink - Mass of sugar
= 110 - 75
= 35 g
Now we can calculate the density:
Density = Mass ÷ Volume
Density = 35 ÷ 100
Density = 0.35 g/ml
The density of soft drink A is indeed 0.35 g/ml.
How do chemical weathering and the formation of biochemical sediment remove carbon from the atmosphere and store it in the geosphere?
Chemical weathering and the formation of biochemical sediment remove carbon from the atmosphere by releasing carbon dioxide through the breakdown of rocks. This carbon dioxide can then be stored in the geosphere as biochemical sediments.
Explanation:Chemical weathering and the formation of biochemical sediment play a crucial role in removing carbon from the atmosphere and storing it in the geosphere. Chemical weathering refers to the breakdown of rocks and minerals through chemical reactions, which releases carbon dioxide into the atmosphere. This carbon dioxide can then be dissolved in water and can react with other compounds to form biochemical sediments, such as calcium carbonate. These sediments eventually become part of the geosphere, storing carbon for long periods of time.
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What volume would 4 moles of gas occupy at stp? do this without a calculator. you may need to use longhand calculations. the question is designed to tolerate reasonable rounding?
The box holds 70 cm3 of water. Water has a density of 10 g/cm³. What is the mass of the water
The number of atoms in 8.93 g of zinc ?
Zinc has a molar mass of about 65.38 g/mol. So we calculate the number of moles first:
moles Zinc = 8.93 g / (65.38 g/mol) = 0.1366 mol
We can calculate for the number of atoms using Avogadros number.
atoms Zinc = 0.1366 mol * 6.022 x 10^23 atoms / mol
atoms Zinc = 8.23 x 10^22 atoms
Assume that 50.0 cal of heat is applied to a 15 g sample of sulfur at 20°C. What is the final temperature of the sample if the specific heat of sulfur is 0.175 cal/(g • °C)?
If a sample containing 2.50 ml of nitroglycerin (density=1.592g/ml) is detonated, how many total moles of gas are produced?
A 0.100 g sample of a carbon–hydrogen–oxygen compound is combusted in a stream of pure oxygen and produces 0.220 g co2 and 0.239 g h2o. what is the mass percent of hydrogen in the sample?
a.13.3
First we assume that the compound containing only C,H,and O is combusted completely in the presence of excess oxygen, so that the only things that can be produced are water and carbon dioxide.
From there we should back calculate the amount of Hydrogen that is in the original sample by taking all of the hydrogen in the 0.239g to came from the organic compound.
And since we know that the original mass of the sample was .100g, we can also easily get a mass % H by taking the mass Hydrogen calculated over the total original mass (.100 g)
So that:
0.239g H2O / (18.01 g/mol) = .01327 moles H20
.01327 Moles H20 * 2.02g H (per every mole H2O) = .0268g H initially present in the sample
.0268g H / .100g sample = 26.8% H by mass
The mass percent of hydrogen in the 0.1 g sample of compound containing carbon–hydrogen–oxygen is 26.6%
We'll begin by calculating the mass of the hydrogen in the compound. This can be obtained as follow:
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Molar mass of H₂ = 2 × 1 = 2 g/mol
Mass H₂O produced = 0.239 g
Mass of H =?Mass of H = [tex]\frac{2}{18} * 0.239[/tex]
Mass of H = 0.0266 gFinally, we shall determine the mass percent of Hydrogen in the compound. This can be obtained as follow:
Mass of H = 0.0266 g
Mass of compound = 0.1
Mass percent of H =?[tex]Percentage = \frac{mass}{mass of compound} * 100\\\\= \frac{0.0266}{0.1} * 100[/tex]
Mass Percent of H = 26.6%Thus, the mass percent of hydrogen in the sample is 26.6%
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A 2.07-g sample of an iron–aluminum alloy (ferroaluminum) is dissolved in excess HCl(aq) to produce 0.100 g H2(g).
Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g)
2Al(s)+6HCl(aq)→2AlCl3(aq)+3H2(g).
What is the percent composition, by mass, of the ferroaluminum?
Final answer:
The percent composition of Fe in the ferroaluminum alloy is approximately 33.82%.
Explanation:
To find the percent composition of the ferroaluminum, we need to determine the mass of iron and aluminum in the alloy. Based on the balanced chemical equations given, 1 mole of Fe is produced for every 2.07 g of the alloy, and 3 moles of H2 are produced for every 2.07 g of the alloy. From the molar mass of Fe (55.85 g/mol) and H2 (2.02 g/mol), we can calculate the mass of Fe and H2 produced. So, the percent composition of Fe in the alloy is:
mass of Fe / mass of ferroaluminum × 100%
= (0.70 g / 2.07 g) × 100%
= 33.82%
Therefore, the percent composition of Fe in the ferroaluminum is approximately 33.82%.
which element on the periodic table contains 5 valence electrons and is a metalloid
Which must be the same when comparing 1 mol of oxygen gas, O2, with 1 mol of carbon monoxide gas, CO?
A. the mass
B. the volume
C. the number of molecules
D. the number of oxygen atoms
What is the mass (in grams) of 9.79 × 1024 molecules of methanol (CH3OH)?
Final answer:
To find the mass of methanol, divide the number of molecules by Avogadro's number to get moles, then multiply by molar mass. The mass of 9.79 × 10²⁴ molecules of methanol is 520.64 grams.
Explanation:
To calculate the mass of 9.79 × 10²⁴ molecules of methanol (CH₃OH), first, we need to determine how many moles of methanol there are. Since 1 mole of any substance contains 6.02 × 10²³ molecules (Avogadro's number), we can use this to find the number of moles:
Moles of methanol =
9.79 × 10²⁴ molecules / 6.02 × 10²³ molecules/mol
This calculation reveals that there are 16.27 moles of methanol. Next, we use the molar mass of methanol, which is 32.0 g/mol, to find the mass:
Mass of methanol = 16.27 moles × 32.0 g/mol = 520.64 grams. Therefore, 9.79 × 10²⁴ molecules of methanol have a mass of 520.64 grams.
A 3.52g sample of chromium metal reacts with fluorine to produce 7.38g of metal fluoride. What is the mass % of Cr in the metal fluoride?
For the reaction 6 Li + N2 → 2 Li3N , what is the maximum amount of Li3N (34.8297 g/mol) which could be formed from 14.18 mol (6.941 g/mol) of Li and 16.37 mol of N2 (28.0134 g/mol)? Answer in units of mol.
The reaction is limited by the amount of Lithium available. With the given amount of Lithium and Nitrogen gas, the maximum amount of Li3N that could be produced is 4.726 moles.
Explanation:The question is looking for the maximum amount of Li3N that can be produced from given amounts of Li and N2. According to the chemical equation 6 Li + N2 → 2 Li3N, six moles of Li react with one mole of N2 to produce two moles of Li3N. Hence, the Li:N2:Li3N mole ratio is 6:1:2. If you have 14.18 moles of Li and 16.37 moles of N2, the reaction is limited by Li because it would require 16.37 moles of N2 to entirely consume 98.22 moles of Li (16.37 moles * 6). But since you only have 14.18 moles of Li, this will limit the formation of Li3N. Therefore, the maximum amount of Li3N that could be produced is 2/6 * 14.18 moles, which equals to 4.726 moles of Li3N.
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The molecular mass of the compound is 90 amu. What is the molecular formula for C2H5O?
First let us get the molecular mass of the compound C2H5O.
C has molar mass of 12 amu, H is 1 amu, while O is 16 amu, therefore:
C2H5O = 12 amu * 2 + 1 amu * 5 + 16 amu = 45 amu
So to get 90 amu, simply double all the elements, therefore:
C4H10O2
Let us assume that the given formula of elements is empirical formula where elements have simplest whole number ratio
The empirical mass = 2 X atomic mass of carbon + 5 X atomic mass of hydrogen + at mass of O
The empirical mass = 2 X 12 + 5 + 16 = 45
The ratio of molecular mass and empirical mass = 90 / 45 = 2
Molecular formula is obtained by multiplying the empirical formula with this ratio / factor
molecular formula = 2 X (C2H5O) = C4H10O2
Give the symbol of the element that has the largest atomic size in group 3a (13).
Final answer:
Thallium, being the heaviest member of Group 13, will have the largest number of electron shells, which makes its atomic radius the largest of the group.
Explanation:
The element in Group 3A (13) with the largest atomic size is thallium, which has the symbol Tl. Atomic size generally increases from top to bottom within a group on the periodic table due to the addition of electron shells.
Thallium, being the heaviest member of Group 13, will have the largest number of electron shells, which makes its atomic radius the largest of the group.
The element with the largest atomic size in Group 3A (13) is thallium (Tl), as atomic size increases down a group.
A kind of sedimentary rock formed from plant material over a long period of time is __________.
What is a substance that contains only a single type of atom
Which two body systems contribute to acid-base balance of blood?
Final answer:
The respiratory and renal systems are crucial in maintaining the acid-base balance of blood, by managing the levels of CO2 and bicarbonate, respectively.
Explanation:
The two body systems that contribute to the acid-base balance of blood are the respiratory system and the renal or excretory system. The primary blood buffer system is carbonic acid/hydrogen carbonate, which aids in maintaining the blood pH within a narrow range. The respiratory system regulates blood pH by exhaling carbon dioxide (CO2), while the renal system adjusts blood pH through the excretion of hydrogen ions (H+) and the conservation of bicarbonate (HCO3-). These two systems play a vital role in the acid-base homeostasis by removing excess acids or bases from the body.
A chemical that causes a sudden, almost instantaneous release of pressure, gas, and heat when subjected to sudden shock, pressure, or high temperatures best describes which type of DOT hazardous materials classification?
Answer:
The correct answer is class I explosives.
Explanation:
An explosive refers to a chemical, which leads to a sudden, almost immediate discharge of gas, pressure, and heat when exposed to sudden pressure, shock, or high temperature. These are unstable substances and are primarily of two kinds.
The type one comprises of substances possessing the tendency of undergoing supersonic reactions, like TNT and nitroglycerin. The other kind comprises substances, which burn briskly, however, at a subsonic rate. The examples are rocket propellants, gunpowder, and fireworks.
How does acetaldehyde impurity arise in the fermentation?
Answer:
Explanation:
Acetaldehyde is a colorless, volatile liquid with a pungent and suffocating smell. It is produced as a result of the oxidation of ethyl alcohol to acid or acetic fermentation. Its formula is: CH3CHO formula.
Acetaldehyde occurs naturally in alcoholic beverages. In excess, however, it resembles the smell and taste of an immature green apple.
Fermentation is a process that degrades molecules to transform them into other simpler molecules.
The most frequent causes for which the impurity of acetaldehyde can be generated in fermentation:
It can be caused by the strain of yeast used. To avoid this, a suitable yeast strain should be chosen for the fermentation process. Due to the premature termination of fermentation: In this case it can occur in two different ways: Due to the depletion of must oxygen due to temperature changes and premature flocculation: Acetaldehyde is an intermediate compound in the formation of alcohol, if fermentation stops at the time of the transformation of glucose into alcohol at the stage of acetaldehyde, it produces a fruity flavor and aroma (green apple). For the exposure of alcohol to oxygen: Causing its oxidation and giving immature green apple flavors. Contamination by infection of the bacterium (acetobacter): It is produced as a byproduct of the end of fermentation when part of ethyl alcohol is transformed due to the action of Acetobacter, a genus of aerobic bacteria. For this reason it is convenient that the oxygen level is low at this stage of the fermentation so that the bacteria do not act.A new element is discovered that is very unstable and highly reactive, and it likes to lose its one valence electron. in what group should this element be placed in? explain.
Which of the following correctly describes the relationship between speed and velocity?
Ions how are ions made from neutral atoms worksheet answers
Final answer:
Ions are created when neutral atoms either lose or gain electrons, forming cations and anions, respectively. The periodic table helps predict the charges of ions depending on their group, where alkali metals form +1 cations, alkaline earth metals form +2 cations, and halogens form -1 anions. The formation of ionic compounds involves the combination of these oppositely charged ions to achieve electrical neutrality.
Explanation:
Ions are formed when atoms gain or lose electrons. When a neutral atom loses one or more electrons from its valence shell, it becomes a cation (a positive ion). Conversely, when it gains one or more electrons in its valence shell, it becomes an anion (a negative ion).
Charges of Ions and Ionic Compounds:
The periodic table can be a tool for predicting the charges of many ions based on their group. For instance, alkali metals form +1 ions, while alkaline earth metals form +2 ions. Halogens typically form -1 ions. Ionic compounds consist of these positive and negative ions in a ratio that balances their total charges, resulting in an electrically neutral compound.
Electron Configurations and Ion Charges:
It's important to note that ions only form through the movement of electrons, not protons. For elements within the same group on the periodic table, the number of valence electrons determines the common ion charge. Elements will either reach a stable electron configuration by losing or gaining electrons to form ions.
At 25 °c and 785 torr, carbon dioxide has a solubility of 0.0351 m in water. what is its solubility at 25 °c and 1510 torr?
The solubility of carbon dioxide in water at 25 °C increases from 0.0351 m at 785 torr to approximately 0.0675 m at 1510 torr.
The solubility of a gas in a liquid is described by Henry's Law, which states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.
Using this law, we can calculate the solubility of carbon dioxide (CO₂) in water at a different pressure while keeping the temperature constant at 25 °C.
At 785 torr, the solubility of CO₂ is 0.0351 m. According to Henry's Law, the solubility (S) can be calculated using the formula S₁/P₁ = S₂/P₂, where S₁ and S₂ are the solubilities at pressures P₁ and P₂, respectively.
If the pressure is increased to 1510 torr, we can find the new solubility (S₂) as follows:
S₂ = S₁ x (P₂/P₁)
= 0.0351 m x (1510 torr / 785 torr)
= 0.0351 m x (1510/785)
= 0.0351 m x 1.9235671
= 0.067533 m (approx)
The solubility of CO₂ at 25 °C and 1510 torr is approximately 0.0675 m.
The main reasons why h2co has a higher vapor pressure at a given temperature when compared to ch3oh is that h2co