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Definition
| The smallest particle of an element that retains its chemical properties and participates in a chemical reaction |
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Term
1. atoms
2. identical, differ
3. created, destroyed, transformed
4. compounds, whole-number
5. constant |
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Definition
Dalton's atomic theory - 5 postulates:
1. An element is composed of extremely small indivisible particles called ____.
2. All atoms of a given element have ____ properties that ____ from those of other elements.
3. Atoms cannot be ____, ____ or ____ into atoms of another element (in normal chemical reactions).
4. ____ are formed when atoms of different elements combine with one another in small ____ ratios.
5. The relative numbers and kinds of atoms are ____ in a given compound. |
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| Elements are made up of ___ and a ____. |
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proton - nucleus, +1 charge
neutron - nucleus, 0 charge
electron - outside nucleus, -1 charge |
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| Name, location and charges of the three basic components of the atom |
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| Mass of an electron is ____ of a proton or a neutron |
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| Since the mass of protons and neutrons is greater than electrons, the majority of the mass of an atom is in the ____. |
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| The diameter of an atom is about ____ times that of its nucleus (so it's mostly empty space!). |
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| The number of ____ determines the identity of an element. |
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| All atoms of a particular element have the same number of ____. |
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| The number of protons of an element is called its ____, or Z. |
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Definition
| An element's atomic number (Z) refers to the number of ___ in the element. |
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Definition
| If the atom is neutral (no charge), then the number of protons and electrons are ____. |
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Term
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Definition
| The sum of the number of protons and neutrons in the nucleus is called the ____ of an atom, or A. |
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Term
A (mass number, or protons + neutrons)
Z (atomic number, or # of protons) |
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Definition
| The number of neutrons in the nucleus is ____ minus ____. |
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Definition
| Atoms can vary in their number of ____ in the nucleus but still be the same type of atom. |
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| False: only the #s of neutrons can vary |
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Definition
| T/F: Atoms can vary in their numbers of protrons in the nucleus, but still be the same type of atom. |
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Definition
| Atoms who vary in the numbers of neutrons in the nucleus are called ____ of each other. |
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| The chemical symbol of isotopes showing the mass number, the atomic number and the chemical symbol |
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| In the periodic table, rows are called ____; columns are called ____. |
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| The ____ shows all the known elements. |
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| The periodic table has ___ groups; elements in groups 1, 2, 13, 14, 15, 16, and 17 are called the ____ elements. |
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| Elements in groups 3-12 are called the ____. |
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Term
(1) alkalai metals
(2) alkaline earth metals
(17) halogens
(18) noble gases |
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Definition
Certain groups in the periodic table have their own names:
Group 1: ____
Group 2: ____
Group 17: ____
Group 18: ____ |
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Term
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Definition
| Elements in the same group have ____ properties (related to reactivity). |
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Term
metals
non-metals
metalloids |
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Definition
| The three main types of elements |
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Term
metalloids
metals
non-metals |
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Definition
| In the periodic table, elements along the diagonal (zig-zag) line are called the ____ (B, Si, Ge, As, Sb and Te); those elements to the left of the diagonal are ____; those to the right are ____. |
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Definition
| T/F: Atoms do occur in nature by themselves (as a pure element), but most atoms combine with others and form compounds. |
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Definition
| When atoms combine with others and form compounds, these compounds exist as either ____ or ____. |
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Definition
| ____ consist of several atoms which come together, share electrons with each other forming covalent bonds, are normally non-metals and are uncharged. |
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Definition
| The molecular or chemical formula shows the chemical composition of the substance and reflects the ___ of the elements present in the molecule or compound. |
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Term
1) 1 H, 1 Cl
2) 2 H, 1 O
3) 1 N, 3 H
4) 3 C, 8 H |
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Definition
How many and which atoms are in the following compounds?
1) HCl
2) H2O
3) NH3
4) C3H8 |
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| Some elements exist not as atoms, but as ____. |
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| ____ formulas are used to show the bonding of atoms to each other. |
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| A ____ structural formula shows the bonding of atoms, but in a shorthand way. |
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Definition
| H2, O2, N2, F2, Cl2, Br2, and I2 are examples of elements that exist as ____ molecules at room temperature. |
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Definition
| Phosphorus occurs naturally as ____ and sulfur as ____ rather than as single atoms. |
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| ____ are formed by the removal or addition of an electron to an atom. |
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| ____ exhibit a "give and take" of electrons rather than a sharing of electrons like molecules. |
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Definition
| Ions are made up of ____ and ____. |
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Definition
| Metals lose electrons to form ____. |
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| Non-metals gain electrons to form ____. |
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Definition
| Whenever an ion is made, positive or negative, the number of ____ NEVER changes; it is only the ____ that move. |
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Definition
| Some ions can be ____ - that is, they consist of more than one atom but carry an overall charge (majority are negative). |
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Definition
| Ions are ____ - not molecules (e.g., can't have a molecule of salt). |
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Definition
| Table salt is a combination of Na+ ions and Cl- ions that are a continuous ____ of ions (i.e,, if you have a Na+ ion, you must also have a Cl- ion). The bonding involved in these structures is known as ____ bonding. |
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Definition
| When writing formulas of the ionic compounds, remember that their overall charge must be ____ (so we combine them so that the number of positive and negative charges are equal). |
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Definition
| T/F: Atoms that are close to the noble gases lose or gain electrons to attain a noble gas electron configuration. |
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Definition
| T/F: Most transition metals can have more than one charge. |
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Definition
| There are only ____ polyatomic cations; the rest are anions. |
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Definition
| Most polyatomic anions contain ____ (called ____). |
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Term
Ammonium (NH4)
Mercury I (Hg2) |
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Definition
| The two polyatomic cations |
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Definition
| Transition metals - assume there is more than one possible charge (except Zn, Cd, and Ag) and will therefore use ____ in the name to describe the charge on the metal. |
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Term
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Definition
| In ionic compounds, the cation is just the name of the ____. |
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Term
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Definition
| In ionic compounds of most transition metals, the name must describe the ____ on the metal (by using ____). |
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Term
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Definition
| In ionic compounds, anions are named by adding the suffix ____ to their non-metal name. O2- is therefore ____; F- is ____. |
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Term
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Definition
| Oxoanions end in ____ and ____ for those that have two oxoanions, with the ____ for the one with the greater number of oxygens. For oxoanions which have more than two possibilities, the prefixes ____ and ____ are also used. |
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Term
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Definition
| ____ compounds consist of two non-metals. |
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Term
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Definition
| In binary molecular compounds (two non-metals), the name consists of the element in the formula that comes ____ followed by the element that comes ____. |
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Term
1) sulfur dioxide
2) sulfur trioxide |
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Definition
Chemical name of these binary molecular formulas:
1) SO2
2) SO3 |
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Term
prefixes
-ide
(e.g. SO2 is sulfur dioxide) |
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Definition
| In binary molecular compounds (two non-metals), ____ are used for each element to determine how many of each is in the molecule and the second element also has the suffix ____. |
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Term
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Definition
| T/F: In binary molecular compounds (two non-metals), if there is only one of the first element, then the prefix mono- is not used. |
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| Some binary compounds form ____ when placed in water because they break apart and form ions. |
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Term
| HCl(aq) hydrochloric acid |
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Definition
| HCl(g) in water solution becomes ____. |
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Definition
| HBr(g) in water solution becomes ____. |
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Term
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| HI(g) in water solution becomes ____. |
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| Polyatomic ions with hydrogen as the cation in water solution can also form ____. The suffix then goes from -ate to ____. |
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