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Soluble ​ ​ The ability of a substance to dissolve in a particular solvent, forming a homogeneous mixture.

easy examples for Given the average atomic mass of an element, find the % abundance of its isotopes Grade 10 SABIS ​ Example 1: Average atomic mass: 15.8 Isotope A mass: 14 Isotope B mass: 16 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 14) + (y * 16) = 15.8 Equation 2: x + y = 100 Solving the equations, we find that x = 40 and y = 60. Answer: Isotope A: 40% abundance Isotope B: 60% abundance Example 2: Average atomic mass: 18.9 Isotope A mass: 17 Isotope B mass: 20 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 17) + (y * 20) = 18.9 Equation 2: x + y = 100 Solving the equations, we find that x = 30 and y = 70. Answer: Isotope A: 30% abundance Isotope B: 70% abundance Example 3: Average atomic mass: 27.5 Isotope A mass: 26 Isotope B mass: 28 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 26) + (y * 28) = 27.5 Equation 2: x + y = 100 Solving the equations, we find that x = 60 and y = 40. Answer: Isotope A: 60% abundance Isotope B: 40% abundance

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Atomic Structure Grade 10 SABIS ​ Nuclear Atom : A nuclear atom is an atom with subatomic particles and a nucleus. Most of it is empty space. Atomic Boundaries : Atoms do not have specific boundaries. Atomic Diameter : The atomic diameter is the distance between two adjacent nuclei. It is in the order of 10^-10 m and it is about 10^4 times the diameter of the nucleus. Nuclear Diameter : The nuclear diameter is in the order of 10^-14 m. Subatomic Particles : Subatomic particles are electrons, protons, and neutrons. Atomic Nucleus : The atomic nucleus contains protons and neutrons (collectively known as nucleons). Comparison Between Subatomic Particles : Proton: +1 charge, 1 amu mass, located inside the nucleus. Neutron: 0 charge, 1 amu mass, located inside the nucleus. Electron: -1 charge, 1/1840 mass of 1 proton, located around the nucleus. Nuclear Atom : In a nuclear atom, the number of positive protons is equal to the number of negative electrons. Nuclear Charge : The nucleus is positively charged since it contains positive protons and neutral neutrons. Atomic Mass : The mass of an atom is concentrated in its nucleus; electrons have negligible mass compared to the nucleus. Neutrons : Neutrons help in binding the nucleus together (prevent protons from repelling each other). Nuclei of Same Element : Nuclei of the same element have the same atomic number (# of protons) and the same nuclear charge Nuclear Atom : Picture an atom as a tiny solar system. The nucleus is the sun, and the electrons are planets orbiting around it. But unlike our solar system, most of an atom is just empty space. It's like if the sun was in New York and the nearest planet was in Los Angeles! Atomic Boundaries : Atoms are like social butterflies. They don't have specific boundaries and are always ready to interact with their neighbors. It's like being at a party where everyone is mingling freely. Atomic Diameter : The atomic diameter is the distance between two adjacent atoms, like two friends standing shoulder to shoulder. It's incredibly small, about 10^-10 meters, which is a hundred million times smaller than the width of a human hair! Nuclear Diameter : The nuclear diameter is even smaller, about 10^-14 meters. That's like comparing the size of a marble to the size of the Earth! Subatomic Particles : Atoms are made up of even tinier particles: protons, neutrons, and electrons. It's like a Lego set, where the individual pieces (subatomic particles) come together to build the final product (the atom). Atomic Nucleus : The atomic nucleus is like the heart of the atom. It's where the protons and neutrons (collectively known as nucleons) live. It's the control center, holding the atom together and defining its identity. Comparison Between Subatomic Particles : Proton: Imagine protons as positive little suns residing in the nucleus. Neutron: Neutrons are the peacekeepers of the atom. They have no charge and hang out in the nucleus, helping to keep the protons from pushing each other away. Electron: Electrons are like speedy little planets orbiting the nucleus. They carry a negative charge and are incredibly light, with a mass about 1/1840 of a proton. Nuclear Atom : In a nuclear atom, the number of positive protons is equal to the number of negative electrons. It's like a perfectly balanced seesaw, with the same weight on both sides. Nuclear Charge : The nucleus carries a positive charge, thanks to the protons it houses. It's like a positive magnet at the center of the atom. Atomic Mass : The mass of an atom is concentrated in its nucleus, just like a peach pit holds most of the peach's weight. Electrons are so light, their mass is almost negligible. Neutrons : Neutrons are like the glue of the atom. They help hold the nucleus together and prevent the protons from repelling each other, just like a mediator in a heated debate. Nuclei of Same Element : Nuclei of the same element have the same number of protons and the same nuclear charge. It's like having a unique ID or barcode that identifies each element.

Each row in the periodic table is called a period while each column is called a group or family. Grade 10 SABIS ​

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Given the average atomic mass of an element, find the % abundance of its isotopes Grade 10 SABIS ​ Given the average atomic mass of an element: It's like having the average weight of a group of people. Isotopes: Think of them as different "versions" of the same element, like having people with varying heights within the group. Each isotope of an element has a specific mass, just like each person in the group has a unique weight. The average atomic mass takes into account the mass of each isotope and their respective abundance in nature, similar to calculating the average weight of a group considering each person's weight and how many people there are of each height. To find the percentage abundance of isotopes, we'll use a formula that involves the average atomic mass and the masses of the isotopes. For example, let's say we have an element with two isotopes: Isotope A with a mass of 10 and Isotope B with a mass of 12. The average atomic mass of the element is given as 11.2. We'll assign variables to the abundance of each isotope, such as x for the abundance of Isotope A and y for the abundance of Isotope B. The average atomic mass is the weighted average of the masses of the isotopes, so we'll set up an equation: (x * 10) + (y * 12) = 11.2. Since the percentages must add up to 100%, we know that x + y = 100. Now, we have a system of two equations: (x * 10) + (y * 12) = 11.2 and x + y = 100. Solving these equations simultaneously, we can find the values of x and y, which represent the percentage abundances of the isotopes. Let's say we find that x = 60 and y = 40. This means that Isotope A makes up 60% of the element's total abundance, while Isotope B contributes 40%. In our everyday lives, we encounter similar situations when analyzing data or determining proportions in various scenarios. For instance, in a bag of assorted candies, finding the percentage of each type is like finding the abundance of isotopes. The average atomic mass provides us with a useful reference point, just as the average weight of a group helps us understand its overall characteristics. By understanding the percentage abundances of isotopes, scientists can gain insights into the natural distribution of elements and how they behave in different contexts. Analyzing the percentage abundances of isotopes is crucial in fields such as geology, chemistry, and forensic science, where precise knowledge of element compositions is essential. In summary, by considering the average atomic mass and the masses of individual isotopes, we can determine the percentage abundances of isotopes, offering a deeper understanding of the element's composition and its significance in various scientific disciplines.

A Balanced Equation Grade 10 SABIS SABIS A chemical equation in which the number of atoms of each element on the reactant side is equal to the number of atoms of the same element on the product side.

The mechanism of a reaction cannot be deduced from net equation of the reaction. Grade 10 SABIS ​

medium difficulty easy examples for Given the average atomic mass of an element, find the % abundance of its isotopes Grade 10 SABIS ​ Example 1: Average atomic mass: 32.7 Isotope A mass: 31 Isotope B mass: 34 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 31) + (y * 34) = 32.7 Equation 2: x + y = 100 Solving the equations, we find that x = 70 and y = 30. Answer: Isotope A: 70% abundance Isotope B: 30% abundance Example 2: Average atomic mass: 42.9 Isotope A mass: 42 Isotope B mass: 44 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 42) + (y * 44) = 42.9 Equation 2: x + y = 100 Solving the equations, we find that x = 60 and y = 40. Answer: Isotope A: 60% abundance Isotope B: 40% abundance Example 3: Average atomic mass: 56.4 Isotope A mass: 55 Isotope B mass: 58 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 55) + (y * 58) = 56.4 Equation 2: x + y = 100 Solving the equations, we find that x ≈ 62.15 and y ≈ 37.85 (rounded to two decimal places). Answer: Isotope A: Approximately 62.15% abundance Isotope B: Approximately 37.85% abundance

dm³ Grade 10 SABIS SABIS A unit of volume equal to one cubic decimeter, equivalent to 1 liter.