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CHEM 6A Lecture Notes - Lecture 2: Unified Atomic Mass Unit, Chemical Reaction, Chemical Formula

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CHEM 6A Full Course Notes

CHEM 6A Full Course Notes

Document Summary

Matter has mass and has volume: consists of atoms and molecules. Examples of non-matter: energy and all of its forms. Atom = the smallest individual particle of an element that maintains its properties. Properties of matter: physical properties are those that can be observed without changing the identity of the substance. Mass: chemical properties are characteristics of substances that are observed as the substance changes into or interacts with another substance(s) Reactivity, flammability, corrosiveness: physical changes are those that occur without changing the identity of the substance. Phase changes, mixing: chemical changes are those that occur when a substance changes into another substance. Types of matter: pure substances are elements and compounds (chemically bonded together, mixtures can be homogeneous or heterogeneous (physically intermingled) Elements: the most basic form of matter, cannot be broken down into simpler substances, all particles that compose an element are virtually identical.

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Related Questions

I need help doing my lab homework, I missed lab that day because, I was sick and it's due.

Chemical Reactions and Equations Learning objectives To observe physical and chemical properties associated with chemical changes To be able to give evidence for the occurrence of a chemical reaction To write a balanced chemical equation To identify areaction as a combination, decomposition, precipitation, single or double replacement, or combustion reaction ntroduction When a substance undergoes a physical change, it changes its appearance but not its composition. For example, when ice melts to form water, it undergoes a physical change from solid to liquid. In a chemical change, the composition of a substance is changed to give a new substance with different physical and chemical properties. For example, when silver tarnishes, the shiny silver (Ag) changes to a dull gray silver sulfide (AgaS). Not only has the chemical formula changed from Ag to Agus, but also the physical properties (shininess) of the substance have changed. Some examples of physical and chemical changes are listed in Table 1 below. Table 1. Comparison of Physical and Chemical Changes Examples of Physical changes Examples and Evidence of Chemical Changes Change in state (melting, freezing, evaporating Formation of a gas (bubbles) subliming) Formation of a solid (precipitate) Change in size Tearing Change in Color Heat is given off or absorbed A solid dissolving in a solvent In a chemical reaction, atoms in the reactants are rearranged to produce new combinations of atoms in the products. However, the total number of atoms of each element in the reactants is equal to the total number of atoms in the products. This is true according to the Law of Conservation of Mass, which states that the total mass remains constant during a chemical reaction. In other words, matter cannot be created or destroyed in a chemical reaction. In a chemical equation, the reactants are shown on the left and the products are on the right. An arrow in between indicates that a chemical reaction occurs. Finally, the physical state of each compound is designated in parentheses after the chemical formula. Solid, liquid, gas, and aqueous (dissolved in water) are shown as(s,(n,(g), and (aq), respectively.

Predict the charge that an aluminum ion would have.

Terms in this set (26)

example of the law of multiple proportions

Two different compounds formed from carbon and oxygen have the following mass ratios:

1.33 g O: 1 g C and 2.66 g O: 1 g C.

2) Which of the following statements is FALSE according to Dalton's Atomic Theory?

A) Atoms combine in simple whole number ratios to form compounds.

B) All atoms of chlorine have identical properties that distinguish them from other elements.

C) One carbon atom will combine with one oxygen atom to form a molecule of carbon monoxide.

D) Atoms of sodium do not change into another element during chemical reaction with chlorine.

E) An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.

The mass number is equal to

the sum of the number of protons and neutrons

a subatomic particle is

A neutral atom contains the same number of protons and electrons

true statement about isotopes

Some elements have 3 or more naturally occurring isotopes

Identify a cation

An atom that has lost an electron

What species is represented by the following information?

p+ = 12 n° = 14 e- = 10

What species is represented by the following information?

p+ = 47 n° = 62 e- = 46

What species is represented by the following information?

p+ = 17 n° = 18 e- = 18

Predict the charge that an aluminum ion would have

Predict the charge that a calcium ion would have

Predict the charge that an ion formed from sulfur would have

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