QUIZ 3.2 Flashcards
nucleus=
SMALL/DENSE/ POSITIVE
_____ orbit the nucleus,
ELECTRONS
atom =
EMPTY SPACE
_____ are orbiting around the
nucleus, accelerating, releasing energy.
ELECTRONS
electrons can only exist in
SHELLS
An electron can exist at
SPECIFIC DISTANCES FROM NUCLEUS
An electron _____be in between
_____levels
CANNOT
ENERGY
The _____is naturally attracted towards
the _____of the atom.
ELECTRON
NUCLEUS
electron absorbs energy=
HIGHER ENERGY LEVEL
If an electron is at a higher energy level, we
say that the electron is
EXCITED STATE
When an electron releases energy, it jumps
to a _____
LOWER ENERGY LEVEL/ GROUND STATE
energy enters the atom=
ELECTRON CAN ABSORB ENERGY BEXOMING EXCITED AND JUMP HIGHER ENERGY LEVELS
When the electron releases the
energy =
ELECTRON RETURNS TO LOWER ENERGY LEVELS
OTHER FORMS OF ELECTROMAGENETIC RADIATION BESIDE VISIBLE LIGHT CAN BE EMITTED
Each energy level can hold
CERTAIN NUMBER OF ELECTRON
The first level can hold
2
the
second can hold
8
and the third
can hold
18
no of e-
2N2
Inside each energy level, there are _____
SUBLEVELS
Inside the sublevels are _____
ORBITALS
Space around a nucleus where an
electron is likely to be found
ORBITALS
Orbitals are NOT _____.
ORBITS
Shape represents =
ELECTRON DENSITY NOT PATH
Each orbital can hold=
2 ELECTRONS
When electrons occupy orbitals =
SPIN ON THEIR AXIS
If 2 electrons occupy an orbital =
SPIN OPPOSITE DIRECTIONS
Arrows are used to symbolize
E-
Electrons exist the in the
SPECIFIC ENERGY LEVELS ( SHELLS)
Inside the energy levels are
SUBLEVELS SPDF
Orbitals are NOT
ELECTRON PATHS
Energy Level – Energy sub level - orbital
A
In the ground state of an
atom, electrons fill atomic orbitals
of the _____ before occupying higher
levels.
LOWEST ENERGY
_____ tells us that if we arrange the elements in order of
increasing atomic number, we periodically encounter elements that have
similar chemical and physical properties.
PERIODIC LAW
Arranged in ____ number
INCREASING ATOMIC NUMBER
columns =
GROUPS
rows =
PERIODS
Elements in a group
SIMILAR PROPERTIES
Group IA:
Group 2A:
Group 6A:
Group 7A:
Group 8A:
Group B:
ALKALI METALS
EARTH METALS
CHALCOGENS
HALOGENS
NOBLE GASES
TRANSITION METALS
57 – 71
LANTHANIDES
89 – 103
ACTINIDES
increases from top to
bottom and decreases from left to right with
respect to position in the periodic table.
METALLIC PROPERTY
Within a group, _____ increase from top to
bottom as _____are added to shells farther
from the nucleus.
ATOMIC RADII
ELECTRONS
Atomic radii decrease from____within a
given period
LEFT TO RIGHT
Down a group, the atomic radii increases because the =
NUMBER OF SHELL INCREASES
Across a period, the charge of the nucleus increases
PULLING ELECTRON CLOSER
_____of
energy required to remove the most loosely
bound electron from an isolated gaseous atom
to form an ion with a 1+
charge.
IONIZATION ENERGY
Ionization energies measure how _____ electrons
are bound to atoms.
TIGHTLY
_____ always requires
energy to remove an electron from the attractive
force of the nucleus.
IONIZATION
Low ionization energies indicate ease
REMOVAL ELECTRONS
_____ is the energy change that
occurs when an electron is added to a
gaseous atom
ELECTRON AFFINITY
Elements with very negative electron
affinities _____
GAIN ELECTRONS EASILY TO FORM NEGATIVE IONS
_____ of an element is a measure of the relative tendency of an atom
to attract electrons to itself when it is
chemically combined with another atom.
EN
ELECTRONEGATIVITY
F is the most _____
ELECTRONEGATIVITY
Noble gases are not ____
ELECTRONEGATIVE
same number proton different number of neutron
ISOTOPES
Atomic mass =
PROTON
NEURTON
who asked “ what makes up everything”
GREEKS
proposed idea that materials are composed of four elements fire/water/air/earth
ARISTOTLE
atomic theory of matter
JOHN DALTON
ENGLISH CHEMIST
METEOROLOGIST
law of conservation mass
ANTOINE LAVOISER
law of definite proportions
JOSEPH PROUST
FRENCH CHEMIST
discovered negative electron
JONJOSEPH THOMSON
designed experiment to study alpha particle
gold foil
ERNEST RUTHERFORD
danish physicist
discovered electron in atom exist in specific region
NIELS BOHR
negatively charged ion
ANION
positively charged ion
CATION
