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88 Cards in this Set
- Front
- Back
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What is a wave? |
In oscillating disturbance by which energy is transferred. |
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What is an oscillating disturbance by which energy is transferred? |
A wave |
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What is the definition of amplitude? |
AKA height. The vertical distance from the midline of a wave to its peak or trough |
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What is the frequency? |
The number of waves that pass a point in one second |
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What is the distance between identical points on successive waves? |
Wavelength |
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What is the rate at which a point on a wave propagates forward |
Speed |
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What is the equation for speed? |
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1.0 Hz is = to.... |
1.0 1wave/s, and 1.0 s^-1 |
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The longer the wavelength the ____ the frequency |
Lower |
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The shorter the wavelength the ____ the frequency |
Greater |
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What is electromagnetic radiation? |
A form of energy exhibiting wavelike behavior as it propagates through space and is the emission and transmission of energy in the form of electromagnetic waves. |
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A form of energy exhibiting wavelike behavior as it propagates through space and is the emission and transmission of energy in the form of electromagnetic waves is.... |
Electromagnetic radiation |
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The higher the frequency the _____ and energy and ____ and wavelength. |
Higher in energy, shorter the wavelength |
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Low frequency has _____ energy and the _____ the wavelength |
Low energy, longer the wavelength |
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The longer the wavelength the _____ frequency and ____ energy |
Low frequency, low energy |
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The shorter the wavelength the ,____ frequency and ____ energy |
High frequency and high energy |
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The energy of light depends on its _____ and _____ |
Frequency and wavelength |
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What is the calculation for speed of light? |
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Speed of light = c = ... |
3.00 x 10^8 m/s |
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What is a continuous or line spectra of radiation emitted by substances? |
Emission spectrum |
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Describe continuous spectra |
All wavelengths, sunlight and heated solids |
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Describe line spectra |
Specific wavelengths, energized gas |
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Each element has its ______ spectra |
Own unique line |
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What are the two different states described in the Neil's Bohr example. |
Ground state and excited state |
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What is ground state? |
Lowest energy level occupied by an electron |
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What is an excited state? |
Energy level of an electron above its ground state |
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What is the force of attraction between oppositely charged ions called? |
Ionic bond |
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What is a compound composed of oppositely charged ions? |
Ionic compounds |
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Compounds forms between metals and nonmetals are ______ |
Ionic compounds |
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To name ionic compounds we give the ____ name followed by the ____ name |
Cation, anion |
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Covalent bonds form between ____ atoms |
Nonmetal |
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In a covalent bond _____ _____ are shared between two atoms |
Two electrons |
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What is drawn between the symbols of two atoms when they share electrons in a covalent bond? |
A dash |
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Covalent compounds form _____ |
Molecules |
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A dash between two chemical symbols indicates a .... |
Covalent bond |
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The _____ group on the periodic table exists as diatomic molecules in their elemental form |
Diatomic |
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Covalent compounds form when... |
Elements combined through covalent bonds forming discrete molecules |
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This is the Lewis structure drawing of water |
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Covalent compounds to fill what role by sharing electrons? |
Octet rule |
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What is the molecular formula? |
Gives the actual number of atoms in the molecule rather than the simplest whole number ratio |
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When naming covalent compounds use ____ to indicate how many atoms are present |
Prefixes |
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Binary covalent compounds are compounds containing... |
Only two elements |
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Metal plus non-metal equals... |
Ionic bond |
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Non-metal plus nonmetal equals |
Covalent bond |
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What formula is used to describe covalent compounds? |
Molecular formulas |
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Molecular formulas indicate... |
The exact number of each atom contained in one molecule |
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To fulfill the octet rule atoms can... |
Either gain or lose electrons to form ions or they can share electrons through covalent bonds |
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What formula do we use for ionic compounds |
Why it's formula unit or empirical formula |
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What is the empirical formula? |
The simplest whole number ratio of cations to anions in compound |
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What is the key to distinguishing between ionic and covalent compounds? |
Identify the elements present |
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Ionic compounds total charge must... |
Equal zero |
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What is the empirical formula. Give example |
Give smallest whole number ratio of atoms in a compound. NaCl |
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What are leftover ions packed together in a structure of alternating positive and negative charges stretched out three dimensions |
Ionic lattice |
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Periodic table and electron rules to remember: The group / column number for the main group is... |
Is the number of valence electrons |
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The periods or row # for the main group tells you... |
The energy level number |
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Columns in the periodic table also correspond to... |
To sub-level electron configurations |
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The main group numbers in the periodic table indicate... |
Number of electrons in each valence level |
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All alkali metals (group 1a) (lose or gain) ___ # of electrons to form +/- ___ ion |
Lose, 1, +1 |
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All alkaline earth metals (group 2a) (lose or gain) ___ # of electrons to form +/- ___ ion |
Lose, 2, +2 |
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Transition metals (d block on pic) (lose or gain) ___ # of electrons to form +/- ___ ion |
Lose, 1-4, positive |
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Nonmetals (halogens) form ____ ions |
-1 |
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Chalcogens ( group 6a ) +/- ____ io s |
-2 |
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Group 5a gain ____ electrons, forma ions of ____ charge |
+3, -3 |
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Cations are... |
Main group metals lose electrons to form pos charged ions |
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Anions are... |
Ned charged ions formed by non metals gaining electrons |
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Which is written first and which is written second and empirical formula |
Cation first then anions |
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What are polyatomic ions? |
Groups of atoms that have an overall charge |
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What are oxyanions |
Polyatomic ions that contain oxygen. |
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What is the rule of thumb when naming oxyanions? |
Add -ate to the root of the element meaning ~ more. Add - ite when indicating ~fewer oxygen atoms present |
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What is the Lewis dot symbols? |
They represent the valence electrons as dots around the atomic symbol |
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What is the octet rule? |
All elements will lose or gain electrons to become like the nearest noble gas and has eight electrons in the valence shell. |
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What does the octet rule explain? |
Explains why noble gases are so stable |
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What are isoelectronics? |
Atoms with the same electron configuration. |
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What is the electron configuration? Give an example. |
Shows the number of electrons in each occupied energy level and sublevel.. 1s^2,2s^2.... |
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What does the electron configuration help determine |
Helps determine how an atom behaves |
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What does this super script in an election configuration tell you |
# of electron resides in the orbital |
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What is an orbital box notation? |
A means of showing the location of electrons in an atom |
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What is the valence shell? |
Outer motel, highest occupied energy level |
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What is the valance electron? |
Electrons in a valence shell |
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What is a Kernel electrons |
Electrons not in a valence shell |
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What does a Bohr model look like? |
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Using the periodic table where can you tell what the valence level is? |
Looking at the row of the periodic table where the element is |
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Using the periodic table how can you tell what the valence electron is? |
Looking at the column of the periodic table where the element is located |
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What does inner electrons mean |
The first two levels in a configuration |
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What are outer electrons? |
Essential to bonding, includes valence level and partially filled D&F sub levels |
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Describe noble gas notation |
Replacing the inner electrons with brackets and the noble gas element symbol |
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Why do we use noble gases to help simplify the electron configuration? |
Because they have complete octets in the inner level |
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What is the hunds rule? |
If empty orbitals of the same energy are available, electrons will singly occupy orbitals rather than pairing up together |
