Shared Flashcard Set

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October flash cards
atomic models and periodic table vocab
50
Chemistry
11th Grade
10/25/2010

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Cards

Term
What is the Quantum leap or atomic spectra process?
Definition
electrons absorb energy and jump up to the excited state -- the release energy as light (colors) and jump down to a lower level
Term
How are metals and nonmetals different?
Definition
metals are good conductors and are usually silver/grey and malleable, but nonmetals are poor conductors and are brittle
Term
What are valence electrons?
Definition
outer shell electrons
Term
When are elements SIMILAR?
Definition
If they are in the same group/ same valence electrons
Term
What is the atomic number?
Definition
number of PROTONS
Term
What is the number of neutrons?
Definition
MASS - Protons
Term
What is an isotope?
Definition
same element, same atomic number, different mass, different neutrons
Term
What is the atomic mass (average)?
Definition
Average of an isotope's masses
Term
What is an ORBITAL?
Definition
a high probability area outside the nucleus where electrons are located
Term
Where are electrons located?
Definition
orbitals
Term
What are nucleons?
Definition
protons and neutrons
Term
What are the numbers of protons and electrons in a neutral atom?
Definition
protons and electrons are the same number in a neutral atom
Term
When an atom loses electrons, what happens to the mass?
Definition
nothing - electrons weigh almost 0 amu
Term
What is the mass of a proton or neutron?
Definition
1 amu
Term
What is Ionization Energy?
Definition
the amount of energy it takes to remove an electron
Term
How does Ionization energy change as you go across a period? Why?
Definition
IE increases as you go across the table because atoms get smaller and hold onto their electrons more tightly. so it takes more energy to remove them
Term
How does Ionization energy change as you go down a group? Why?
Definition
IE decreases as you go down the table because atoms get larger and hold onto electrons more loosely, so it takes less energy to remove them
Term
How does Atomic Radius change as you go across a period?
Definition
Radius gets smaller as you go across because the nucleus pulls the electrons into more closely and more tightly
Term
How does Atomic Radius change as you go down a period?
Definition
Radius gets larger as you go down a group because there are more shells and the electrons are held more loosely
Term
How do you draw an atom?
Definition
Draw the nucleus and write the protons and neutrons inside. Then draw the shells/rings and use the electron configuration from the periodic table to put the electrons in the shells.
Term
How do you draw a LEWIS diagram?
Definition
Write the symbol and put the dots to represent the VALENCE (outer) electrons only
Term
What is electronegativity?
Definition
The ability to attract electrons
Term
What are NOBLE gases?
Definition
group 18 gases - they are full and happy - they do not react usually also zero electronegativity
Term
What are HALOGENS/ HALIDES?
Definition
Group 17 fluorine, chlorine, etc
Term
What 2 things did Rutherford learn from his GOLD FOIL experiment?
Definition
atoms are mostly empty space and atoms have a tiny, dense nucleus
Term
Which particle is negative?
Definition
electrons
Term
Which particles have the same mass?
Definition
protons and neutrons
Term
Which particle is positive?
Definition
proton
Term
Which particle is neutral?
Definition
neutrons
Term
Which side of the Periodic Table are metals usually found?
Definition
left
Term
Which side of the Periodic Table are nonmetals usually found on?
Definition
right
Term
What subatomic particle has almost no mass?
Definition
electron
Term
how do you calculate the number of neutrons?
Definition
mass number - atomic number
Term
How do you know mass number?
Definition
It is given in the notation
Term
How do you find atomic number ?
Definition
It is on the periodic table.
Term
How do you find number of protons?
Definition
same as atomic number
Term
How do you find the number of electrons?
Definition
it is the same as protons. Atoms are neutral so positive and negative must balance.
Term
How do you know if elements are isotropes?
Definition
they have the same element symbol, same atomic number, but different mass and different neutrons
Term
How do you know if elements are allotropes?
Definition
They are the same element, but different formulas, shapes, structures, properties
Term
Where do I find the ground state e- configuration?
Definition
on the periodic table
Term
What is the excited state?
Definition
when an e- has absorbed energy and jumped up a level.
Term
What si the difference between quantitative and qualitatitve?
Definition
quantitative is number data; qualititative is descriptive
Term
What is the difference between an observation and an inference?
Definition
Observations are facts gained from your 5 senses; inferences are your Ideas/thoughts about your observations
Term
What are the 7 diatomics?
Definition
H2,O2, N2, F2, Cl2, Br2, I2
Term
how do you calculate the number of neutrons?
Definition
mass number - atomic number
Term
Why are metals good for pots and pans?
Definition
they conduct heat well , to cook the food evenly
Term
Why are metals used for wires?
Definition
metals are ductile and conduct electricity well because metals lose e- easily which allows electricity to flow
Term
What is Ionization Energy?
Definition
the amount of energy it takes to remove an electron
Term
In Rutherford's experiment , MOST of the alpha particles went through UNDEFLECTED, this meant…
Definition
that atoms were mostly empty space
Term
In Rutherford's experiment, A FEW of the alpha particles were repelled backward and scattered, this meant…
Definition
that atoms have a small dense core in the middle called the nucleus
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