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153 Cards in this Set
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Define chemistry |
The study of the composition of matter and the changes that matter undergoes. |
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What is matter? |
Anything that has mass and occupies space. |
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_________ is a measure of the amount of matter that an object contains. |
Mass (measured in standard international (SI) unit of kilograms) |
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What is weight and how do we measure it? |
Weight is the force with which the earth pulls on an object. It is measured in standard international (SI) unit Newtons. |
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What are the 5 branches of chemistry? |
Inorganic, organic, analytical, physical and biochemistry. |
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The study of chemicals that do not contain carbon is called? |
Inorganic chemistry. |
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Define organic chemistry. |
The study of chemicals that contain carbon. Basically the study of chemicals in living organisms. |
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What do we call the study of the composition of matter? |
Analytical chemistry |
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This branch of chemistry studies the mechanisms, rate and energy transfer that happens to matter when it undergoes change. |
Physical chemistry |
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____________ explores the chemical processes within and related to living organisms. |
Biochemistry |
Digestive enzymes, milk formation, hormones. |
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What is the difference between science and technology? |
Science is the study of something, while technology is the application of that science. |
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What is microscopic? |
Objects that can only be seen with a microscope. |
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Objects that can be seen without the help of a microscope are called? |
Macroscopic |
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Aristotle, a philosopher in 4th century BC Greece believed what 2 important concepts? |
That there are 4 elements (earth, water, air and fire) and that matter is perpetually divisible. |
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Who was the father of the first atomic theory and told us that the atom is indivisible? |
Democritus, 4th century BC Greece |
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What group of people developed the first lab equipment in their quest to change common metals into gold and develop medicine? |
Alchemists |
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What was Italian scientist Galileo Galilei's claim to fame? |
The father of the scientific method (along with English scientist Francis Bacon) |
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Who is regarded as the father of modern chemistry? |
Antoine Lavoisier. |
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What did Antoine Lavoisier discover? |
Nitrogen, the law of conservation of mass. Also designed lab equipment and used observation and measurements, along with data analysis. |
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Who was John Dalton? |
Founded modern atomic theory, told us all matter is made of atoms. |
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What is Amedeo Avogadro famous for? |
Avegadro's Number - 6.02x10²³ (one mole of any substance contains 6.02x10²³ particles) |
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Who was the father of the periodic table? |
Dmitri Mendeleev |
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What is the scientific method? |
The steps followed during the scientific process. |
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Observation, hypothesis, experiment/study, theory and law are the steps of what? |
The scientific method. |
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A well tested scientific explanation for a broad set of observations is called? |
Theory |
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__________ is a summary of results that does not explain them. Can change or be abandoned when contradicted by new experiments. |
Law |
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What is observation? |
The recognition of a problem. |
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A hypothesis is described as? |
A proposed explanation of an observation that is based on scientific background and can be tested. |
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What is the experiment or study phase of the scientific method? |
When we use a set procedure to test a hypothesis. |
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All ___________ is made of elements. |
Matter |
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How many elements are there? |
118 known. |
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How many elements make up most of the known matter in our world? |
88. |
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An element is described as what? |
The smallest unit of matter that cannot be broken into smaller units. |
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_________ are either pure or make up what are called compounds. |
Elements. |
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Describe the difference between an atom and an element. |
An atom will have the same number of protons and electrons. An element is a substance made entirely of one type of atom. |
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What are the parts of an atom? |
Electons, protons and neutrons. |
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What are the principles of naming elements? |
Always written in one or two letter abbreviations, only the first letter is capitalized. |
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When was the periodic table originally created, and by whom? |
In 1872 by Russian scientist Dmitri Mendeleev. |
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How many elements were on the first periodic table? |
60 |
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How is the periodic table made and organized? |
By atomic structure, atomic number and chemical and physical properties. |
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The periodic table was created to: |
Put elements in rows of increasing atomic weight and in columns by the way they react. |
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What is each horizontal row of the periodic table called? |
A period. Periods are counted as 1 to 7 from top to bottom. |
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The vertical columns of the periodic table are called ___________ and are characterized by having similar chemical properties. |
Groups or families. |
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What are the representative elements? |
Elements in the first 2 and last 6 groups on the periodic table. |
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What do we call the middle 10 groups on the periodic table? |
Transition elements. |
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What is the name for elements in Group 1A? |
Alkali metals (except hydrogen). |
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What are the alkaline earth metals? |
Elements in group 2A that are shiny but non reactive metals. |
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____________ are highly reactive elements in group 7A. |
Halogens. |
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The inert, non reactive gases in group 8A are called? |
Noble gases. |
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What is the zig zag line that separates metals from non metals on the periodic table? |
The metalloid. |
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What are the characteristics of metals? |
Shiny solids that are good conductors of heat and electricity. They are solid at room temperature (except mercury) with a high melting point and high density. |
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Shiny ductile or malleable elements that are poor conductors and have a low melting point and density are called? |
Non-metals. |
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What are metalloids? |
A group of elements that have some characteristics of both metals and non-metals. They are all semi-conductors and can be modified to be good conductors or insulators. |
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What is Dalton's Atomic Theory? |
Atoms are the building blocks of the element. Atoms are all similar in the same element. Atoms are not similar in different elements. Two or more different atoms may bind in simple ratios to form compounds. A chemical reaction involves the rearrangement, separation or combination of atoms. Atoms are never created or destroyed in a chemical reaction. |
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What are the subatomic particles? |
Electron, proton, neutron. |
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What is the basic charge of an electron and it's relative mass? |
1- and 0 amu. |
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___________ have a 1+ charge and a relative mass of 1 amu. |
Protons. |
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Neutrons have a _________ charge and a relative mass of ______ amu. |
0, or neutral charge. 1 amu. |
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What is the diameter of the nucleus of an atom? |
10‐¹⁵m |
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10‐²⁸g is the mass of what? |
An electron |
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The mass of a proton is |
10-²⁴g |
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What is an atomic mass unit (amu)? |
1/12th of the mass of a carbon atoms, which has a nucleus containing 6 protons and 6 neutrons. |
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What is another name for an amu in biology? |
A Dalton, after John Dalton. |
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On the amu scale, what 2 things have a mass of approximately 1 amu? |
Protons and neutrons. |
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What are the defining features or a proton? |
They have a positive charge and determine the element. |
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What has no charge and helps us determine an isotope? |
Neutrons. |
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Describe electrons. |
They have a negative charge, participate in chemical reactions, and the valence electrons determine chemical behaviour. |
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What 2 things are found in the nucleus of an atom? |
Protons and neutrons. |
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What is the atomic number? |
The number of protons in an atom. |
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All atoms of an element have the same number of protons, true or false? |
True. |
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Where do we find the atomic number on the periodic table? |
Above the elemental symbol. |
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The number of protons + neutrons in an atom is called? |
The mass number. |
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How many electrons are in an atom and why? |
The number of electrons is equal to the number of protons in an atom, because the atoms always has a net neutral charge (not always true of an ion). |
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An ___________ is an atom with the same number of protons, but a different number of neutrons. |
Isotope. |
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What is the key difference between an atom and it's isotopes? |
The mass number (protons+neutrons). |
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How do we name an isotope? |
For their mass number. Ex. Chlorine-35 and Chlorine-37. |
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What is atomic mass? |
The weighted average mass of all the atomic masses of the isotopes of an atom. |
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Where do we find atomic mass on the periodic table? |
Usually right below the atomic symbol. |
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Electrons of the same energy group are in the same ___________ |
Energy level. |
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How are the energy levels assigned? |
Numbers from 1-7, depending on how close the are to the nucleus. |
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Describe atomic spectrum. |
When light from an element that is heated passes through a prism, it separates into distinct lines of colour, which is unique to each element. |
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The ____________ electron energy levels hold fewer electrons. |
Lower. |
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Electrons can run between the energy levels, true or false? |
False. They can never run between the levels, the must flow at their specific energy level. |
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For an electron to move from low energy to higher energy levels, it will need _____________. The opposite is also true. |
Energy. |
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The ________________ needed or emitted is equal to the difference between two energy levels. |
Amount of energy. |
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The first 20 elements are _____________ and follow ____________. |
Consistent, the rules of arrangement. |
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The lowermost energy level can hold how many electrons? |
2 |
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How many electrons can be held in each energy level, starting closest to the nucleus? |
2, 8, 8 (18), 18, 18, 32, 32 |
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The ___________________ of atoms is a major determinant for both chemical and physical properties of elements. |
Electron arrangement. |
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What are the trends in the periodic table? |
Group number and valence electrons, electron-dot symbol, atomic size, ionization energy, metallic character. |
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Describe valence electrons. |
Those electrons found in the outermost energy level. |
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The chemical properties of elements in groups 1A to 8A are mostly due to? |
The valence electrons. |
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What gives us the number of valence electrons on the periodic table? |
The group number. |
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What is the alternative name for the Electron-Dot Symbol? |
The Lewis Structure. |
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What does the Electron-Dot Symbol represent? |
The valence electrons as dots placed on the top, sides and bottom of the elemental symbol. |
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When using the Electron-Dot Symbol, if the number of electrons is greater than 4, what happens? |
Dots are paired. |
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What is another name for atomic size? |
Atomic radius. |
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How do we determine atomic size? |
The distance from the valence electrons to the nucleus. |
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What two factors affect atomic size? |
Atomic number and the balance between attractions and repulsions in the atom. |
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As attraction between the positive nucleus and negative valence electrons increases, atomic size ____________. |
Decreases. |
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How does the atomic size change from left to right on the periodic table? |
It decreases, as there is an increase in nuclear charge (ENC) |
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What is ENC? |
Effective Nuclear Charge - the number of protons - the number of CORE electrons. |
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Why is the size of an atom different from the size of its ion? |
Ions have gained or lost electrons in the valence shell, so the pull of the positive nucleus on the negative electrons is altered. |
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What is ionization energy? |
The energy required to remove an electron from a gaseous atom. |
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If the number of electrons is small and the ENC is large, electrons will be difficult to remove. Why? |
The ionization energy is high. |
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Why is it harder to remove a second electron than the first? |
Because the number of electrons is reduced, but the ENC doesn't change. The pull on the electrons is now greater. |
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Noble gases have __________ and ______ energy levels. |
Stable and high. |
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In general, ionization energy is low for what type of element? |
Metals. |
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What is the ionization energy like for non-metals? |
High, very difficult to remove electrons. |
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An element that has a metallic character loses ____________ easily. |
Valence electrons. |
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What is more prevalent on elements in the left side of the periodic table than on the right? |
Metallic character. |
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Metalloids lose electrons, but to a lesser extent than? |
Metals. |
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How does metallic character change from top to bottom and why? |
It increases from top to bottom as the number of electrons is larger the further down the table you get. |
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What is an ion? |
An element that has gained or lost one or more electrons. |
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How does an atom lose or gain electrons? |
To or from another element. |
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When losing or gaining electrons, how is the charge of the ion impacted? |
When losing, the element becomes positively charged (there are more protons than electrons now). When gaining, the element become negatively charged (there are more electrons than protons) |
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What is another name for positively charged elements? |
Cations (usually a metal) |
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What is an Anion? |
A negatively charged element (usually a non metal) |
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Describe the octet rule |
All atoms have the tendency to attain the noble gas electron arrangement, with the outermost energy level full. |
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How do we write an ions charge? |
To the top right of the atomic symbol. We also write the number of electrons that are lost or gained if more than one. Ex. Al+3, Na+ |
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How can we use group number to determine ionic charge? |
For a metal, the number of charges is equal to the group number. For non-metals, the number of charges is equal to the group number minus 8. (If using 1-18) |
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What is an ionic compound? |
Positive and negative ions connected together by ionic bonds. |
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Most compounds are ________ at room temperature. |
Solid. |
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Describe an ionic bond |
When two elements bond through the giving and receiving of valence electrons. |
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How do we communicate a compounds makeup? |
By using atomic symbols, followed by the number of that element needed to fulfill the octet rule. Ex. MgCl2 |
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The charge of an ________________ should always be zero |
Ionic compound. |
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Why do ions bond ionically? |
To fulfill the octet rule and become stable. |
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What is the formula unit? |
The lowest ratio of ions in an ionic compound. |
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What comes first when naming ionic compounds, the metal or the non-metal? |
The metal. |
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True or false; when naming an ionic compound, the name of the metal part of the compound is not changed. |
True. |
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What suffix do we use for the non-metal component of an ionic compound? |
-ide |
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Do we mention subscripts when naming ionic compounds? |
No, as it will be understood by charge balance. |
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What is a variable charge metal? |
A metal that can form more than one ion form. |
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Where do we find most variable charge metals? |
Mostly the metals in the transition elements. |
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Why do we use roman numbers when writing elemental ions? |
To distinguish the charge level of variable charge ions. |
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What is the charge of Iron (III)? |
3+ |
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What is the equation for charge balance? |
# of Anions and charge + # of Cations and charge = 0 |
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We use charge balance to help us determine what? |
The ionic charge of a variable charge ion. |
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What is the structure for writing the formula of an ionic compound? |
Atomic symbol for the metal with subscript, followed by the non-metal with subscript. |
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What are polyatomic ions? |
A group of atoms that has an overall ionic charge, usually consisting of non-metals bonded to oxygen. |
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True or false, most polyatomic ions consist of cations? |
False. The are made of non-metals, or anions. |
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What is the one polyatomic ion with a positive charge? |
NH4+ |
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What are the 2 suffixes for polyatomic ions? |
-ate and -ite |
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When would you use the suffix -ite for a polyatomic ion? |
When the related ion has one less oxygen. |
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Like any other ion, _________ are bonded with another ion of an opposite charge. |
Polyatomic ions |
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How does a polyatomic ion behave? |
Exactly like any single ion in a compound. It desires to become a zero charge compound. |
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What is the covalent bond? |
When atoms form molecules by sharing electrons. Only done between non-metal atoms. |
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What are the steps to writing dot structures for covalent bonds? |
1. Skeleton molecule with the lone atom in the middle. 2. Find number of electrons needed to fulfill octet rule. (N) 3. Find the number of valence electrons you have. (H) 4.Subtract to find the number of bonding electrons (B) (N-H=B) 5. Subtract again to find non-bonding electrons (H-B=NB) 6. Insert minimum number of B, adding until you have them all. 7. Insert non-binding electrons around, not between. |
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How to we name a covalent compound to describe the number of ions in the anion? |
Mono-, Di-, Tri-, Tetra-, Penta-, etc. |
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In a covalent compound, _________ is the first part of the formula and is given its elemental name. |
The first non-metal |
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What do we give the suffix -ide? |
The second non-metal of a covalent compound. |
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Why do we use prefixes in naming covalent compounds? |
Because several compounds share the same two non-metals. |
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