Chapter 1 Learning Objective Summary
... Chemical reactions involve the gain, loss, or sharing of the outer electrons, whereas nuclear reactions involve changes to the composition of the nucleus. This means that alchemy is possible (though not economical!), because transmutation of one element into another can be accomplished via radioacti ...
... Chemical reactions involve the gain, loss, or sharing of the outer electrons, whereas nuclear reactions involve changes to the composition of the nucleus. This means that alchemy is possible (though not economical!), because transmutation of one element into another can be accomplished via radioacti ...
Unit 2 - Chapter 3 Elements, Atoms, Ions The elements Can we
... always has the same composition regardless of where it comes from or how it is made ...
... always has the same composition regardless of where it comes from or how it is made ...
Biology – The Living Environment
... present at each level. Understand how and why nutrients cycle through the environment (p. 48), you can expect to have to draw a diagram that shows how materials cycle through the environment (53-57) Understand what a symbiotic relationship is and the three different types that are recognized (44-45) ...
... present at each level. Understand how and why nutrients cycle through the environment (p. 48), you can expect to have to draw a diagram that shows how materials cycle through the environment (53-57) Understand what a symbiotic relationship is and the three different types that are recognized (44-45) ...
Chapter 3 PowerPoint
... Law of multiple proportions States that if two or more different compounds are composed of the same elements, they always combine in small whole number ratios. Example: The element carbon and oxygen can combine to form two different compounds, carbon monoxide and carbon dioxide. In carbon monoxid ...
... Law of multiple proportions States that if two or more different compounds are composed of the same elements, they always combine in small whole number ratios. Example: The element carbon and oxygen can combine to form two different compounds, carbon monoxide and carbon dioxide. In carbon monoxid ...
Periodic Table Vocabulary Periodic Table – a chart that organizes
... Valence Electrons – electrons that are located in the outermost principle energy level of an atom. Electron Cloud – the region surrounding the nucleus of an atom where the electrons are located. Ion – an atom that has gained or lost one or more electrons. Ionic Bond – a bond formed by the transfer o ...
... Valence Electrons – electrons that are located in the outermost principle energy level of an atom. Electron Cloud – the region surrounding the nucleus of an atom where the electrons are located. Ion – an atom that has gained or lost one or more electrons. Ionic Bond – a bond formed by the transfer o ...
Name Objective 1: Matter and Energy C3H8 + 5O2 → 3CO2 + 4H2O
... 5.32 g/cm3; germanium; metalloid 7.87 g/cm3; iron; metal 11.3 g/cm3; lead; metal 13.6 g/cm3; mercury; metal ...
... 5.32 g/cm3; germanium; metalloid 7.87 g/cm3; iron; metal 11.3 g/cm3; lead; metal 13.6 g/cm3; mercury; metal ...
Matter
... Consists of only one kind of atom, • Cannot be broken down into a simpler type of matter by either physical or chemical means • Can exist as either atoms or molecules. ...
... Consists of only one kind of atom, • Cannot be broken down into a simpler type of matter by either physical or chemical means • Can exist as either atoms or molecules. ...
ATOMIC THEORY
... 3. Law of Multiple Proportions- if two or more different compounds are composed of the same two elements, then the ratio of the masses is always a ratio of small whole numbers. (John Dalton 1804) C. Dalton’s Atomic Theory 1. In 1810, Dalton published the ideas of the atomic theory, explaining that a ...
... 3. Law of Multiple Proportions- if two or more different compounds are composed of the same two elements, then the ratio of the masses is always a ratio of small whole numbers. (John Dalton 1804) C. Dalton’s Atomic Theory 1. In 1810, Dalton published the ideas of the atomic theory, explaining that a ...
Classifying Matter and the Periodic Table
... Dalton’s atomic theory of matter • each element is composed of extremely small particles called atoms • all atoms of a given element are identical, but they differ from those of other any other element ...
... Dalton’s atomic theory of matter • each element is composed of extremely small particles called atoms • all atoms of a given element are identical, but they differ from those of other any other element ...
Page 233 - ClassZone
... claimed that all matter was made of tiny particles he called atoms. Democritus said that all atoms were made of the same material. The objects of the world differed because each was made of atoms of different sizes and shapes. How does the modern view of atoms differ from this ancient view? How is i ...
... claimed that all matter was made of tiny particles he called atoms. Democritus said that all atoms were made of the same material. The objects of the world differed because each was made of atoms of different sizes and shapes. How does the modern view of atoms differ from this ancient view? How is i ...
Lecture 3
... Isotopes are atoms of the same element that have different mass numbers; they have the same number of protons but different numbers of neutrons Isotopes are difficult to separate from each other, therefore they occur in any sample of the element in their natural abundance which remains relatively co ...
... Isotopes are atoms of the same element that have different mass numbers; they have the same number of protons but different numbers of neutrons Isotopes are difficult to separate from each other, therefore they occur in any sample of the element in their natural abundance which remains relatively co ...
Ch2 lecture outline - OnCourse Systems For Education
... 4. How many (total) periods are on the periodic table? ...
... 4. How many (total) periods are on the periodic table? ...
Summative Assessment Study Guide Name: Due date: SPS1
... SPS3. Students will distinguish the characteristics and components of radioactivity. a. Differentiate among alpha and beta particles and gamma radiation. b. Differentiate between fission and fusion. c. Explain the process half-life as related to radioactive decay. d. Describe nuclear energy, its pra ...
... SPS3. Students will distinguish the characteristics and components of radioactivity. a. Differentiate among alpha and beta particles and gamma radiation. b. Differentiate between fission and fusion. c. Explain the process half-life as related to radioactive decay. d. Describe nuclear energy, its pra ...
CHAPTER 1 Practice Exercises 1.1 12.3 g Cd 1.3 26.9814 u 1.5
... A compound is a chemical species comprised of two or more elements in a definite and unchanging proportion. A reactant is a chemical species which is transformed in a chemical reaction A chemical reaction is a process whereby one or more chemical species is/are transformed into different chemical sp ...
... A compound is a chemical species comprised of two or more elements in a definite and unchanging proportion. A reactant is a chemical species which is transformed in a chemical reaction A chemical reaction is a process whereby one or more chemical species is/are transformed into different chemical sp ...
Semester 2 Chemistry and Matter 1/25
... 2. Substances that cannot be broken into simple substances by chemical means Most Common Elements in Earth’s Crust 46.6% Oxygen (O) 27.7% Silicon (Si) 8.1% Aluminum (Al) 5.0% Iron (Fe) 3.6% Calcium (Ca) 2.8% Sodium (Na) 2.6% Potassium (K) 2.1% Magnesium (Mg) ...
... 2. Substances that cannot be broken into simple substances by chemical means Most Common Elements in Earth’s Crust 46.6% Oxygen (O) 27.7% Silicon (Si) 8.1% Aluminum (Al) 5.0% Iron (Fe) 3.6% Calcium (Ca) 2.8% Sodium (Na) 2.6% Potassium (K) 2.1% Magnesium (Mg) ...
CHAPTER 1 Practice Exercises 1.1 x = 12.3 g Cd 1.3 2.24845 ×12 u
... definite ratios as atoms. This guarantees that elements combine in definite mass ratios, assuming the atoms are indestructible. ...
... definite ratios as atoms. This guarantees that elements combine in definite mass ratios, assuming the atoms are indestructible. ...
Vocabulary and Section Summary
... Name ______________________________ Class___________________Date__________________ ...
... Name ______________________________ Class___________________Date__________________ ...
Chapter 2
... Elements and Compounds 1. Distinguish between an element and a compound. 2. Identify the four elements that make up 96% of living matter. 3. Define the term trace element and give an example. Atoms and Molecules 4. Draw and label a simplified model of an atom. Explain how this model simplifies our u ...
... Elements and Compounds 1. Distinguish between an element and a compound. 2. Identify the four elements that make up 96% of living matter. 3. Define the term trace element and give an example. Atoms and Molecules 4. Draw and label a simplified model of an atom. Explain how this model simplifies our u ...
Keypoints of Basic Atomic Structure
... Atomic Number Atomic Radius Electrons Element Isotope Neutrons Periodic Table Protons Subatomic Particles Concepts 1. Be able to describe how protons, neutrons and electrons are arranged in an atom. 2. Be able to list the charges on the subatomic particles that make up and atom, and giv ...
... Atomic Number Atomic Radius Electrons Element Isotope Neutrons Periodic Table Protons Subatomic Particles Concepts 1. Be able to describe how protons, neutrons and electrons are arranged in an atom. 2. Be able to list the charges on the subatomic particles that make up and atom, and giv ...
answers
... d.) Bohr – solar system model of atoms, energy levels at increasing distance from nucleus ...
... d.) Bohr – solar system model of atoms, energy levels at increasing distance from nucleus ...
ch2_objectives
... 4. Draw and label a simplified model of an atom. Explain how this model simplifies our understanding of atomic structure. 5. Distinguish between each of the following pairs of terms: a. neutron and proton b. atomic number and mass number c. atomic weight and mass number 6. Explain how the atomic num ...
... 4. Draw and label a simplified model of an atom. Explain how this model simplifies our understanding of atomic structure. 5. Distinguish between each of the following pairs of terms: a. neutron and proton b. atomic number and mass number c. atomic weight and mass number 6. Explain how the atomic num ...
Chemical element
A chemical element (or element) is a chemical substance consisting of atoms having the same number of protons in their atomic nuclei (i.e. the same atomic number, Z). There are 118 elements that have been identified, of which the first 94 occur naturally on Earth with the remaining 24 being synthetic elements. There are 80 elements that have at least one stable isotope and 38 that have exclusively radioactive isotopes, which decay over time into other elements. Iron is the most abundant element (by mass) making up the Earth, while oxygen is the most common element in the crust of the earth.Chemical elements constitute approximately 15% of the matter in the universe: the remainder is dark matter, the composition of it is unknown, but it is not composed of chemical elements.The two lightest elements, hydrogen and helium were mostly formed in the Big Bang and are the most common elements in the universe. The next three elements (lithium, beryllium and boron) were formed mostly by cosmic ray spallation, and are thus more rare than those that follow. Formation of elements with from six to twenty six protons occurred and continues to occur in main sequence stars via stellar nucleosynthesis. The high abundance of oxygen, silicon, and iron on Earth reflects their common production in such stars. Elements with greater than twenty six protons are formed by supernova nucleosynthesis in supernovae, which, when they explode, blast these elements far into space as planetary nebulae, where they may become incorporated into planets when they are formed.When different elements are chemically combined, with the atoms held together by chemical bonds, they form chemical compounds. Only a minority of elements are found uncombined as relatively pure minerals. Among the more common of such ""native elements"" are copper, silver, gold, carbon (as coal, graphite, or diamonds), and sulfur. All but a few of the most inert elements, such as noble gases and noble metals, are usually found on Earth in chemically combined form, as chemical compounds. While about 32 of the chemical elements occur on Earth in native uncombined forms, most of these occur as mixtures. For example, atmospheric air is primarily a mixture of nitrogen, oxygen, and argon, and native solid elements occur in alloys, such as that of iron and nickel.The history of the discovery and use of the elements began with primitive human societies that found native elements like carbon, sulfur, copper and gold. Later civilizations extracted elemental copper, tin, lead and iron from their ores by smelting, using charcoal. Alchemists and chemists subsequently identified many more, with almost all of the naturally-occurring elements becoming known by 1900. The properties of the chemical elements are summarized on the periodic table, which organizes the elements by increasing atomic number into rows (""periods"") in which the columns (""groups"") share recurring (""periodic"") physical and chemical properties. Save for unstable radioactive elements with short half-lives, all of the elements are available industrially, most of them in high degrees of purity.