LECTURE 3 Flashcards
____ the attractive force of an element for a shared pair of electrons in a molecule.
– Trend
• Non Metals form ____ by gaining electron high electronegativity
• Metals form ____ by losing electron low electronegativity
•Increases from ____ along the period
• ____ from top to bottom in groups or families
Electronegativity
Anion
Cation
Left to right
Decreases
– Have the same number of electrons,
thus, they have the same electronic
configurations
– Differs in the nuclear charges
Isoelectronic species
- The amount of energy released or absorbed when an electron is added to an atom to form
a negative ion
– A measure of the attraction of an atom for an electron or the atom’s tendency to form a negative ion
Electron affinity
– Is the energy required to remove an electron from an atom.
– Trend
• ____ from top to bottom in groups and families
•_____ from left to right (with some irregularities
Ionization energy
Decreases
Gradual increase
– Specific patterns that are present in the periodic table that illustrate different aspects of a certain element
Periodic properties of elements
Classification of Elements by block
– ____ Elements/Metals (B Group)
• Also known as ____ elements
• Characterized by their electrons filling the d orbital
– _____ element
• Also known as ____ Elements
• Characterized by their electron filling the f orbital
Transition elements
D- transition
Inner transition elements
F- transition
– ____ (Group 8A)
• Also known as ____
because no chemical reactions
were known for them
– _____ Elements (A Group)
• Their last Electron is assigned to
an outer shell s or p orbital
Noble gases
Inert gases
Representative elements
____ States that when elements are arranged in order of increasing atomic number, their physical and chemical properties
show a periodic pattern
• ____
– Each rows are called ____
– Each column are called ___ or
Families which shares similar chemical properties
Periodic law
Periodic table
Periods
Groups
_____Assignment of all of the electrons in an atom into specific shells and subshells
– Designation
•____ = principal quantum number, n
•____ = angular quantum number, (s, p, d or f)
• _____ = superscript number
Electron configuration
Shell
Subshell
Number of electrons
No ____ electrons can occupy one
orbital.
____occupy the lowest possible energy sublevels; they enter a higher sublevel only when the lower sublevels are filled._
____ in a given sublevel of equal energy are each occupied by a single electron before a second electron enters them.
More than two
Electrons
Orbitals
– Is primarily based on the
wave properties of matter
and it describes the behaviour of very small particles
Quantum mechanics
____ an atom or a group of atoms that has a positive or negative charge
– Classified as:
• ____ – an ion with a positive net charge
• ____ – an ion with a negative net charge
Ions
Cation
Anion
___Elements that consist of different masses.
a given element contain the same number of protons ( and also the same number of electrons) because they are atoms of the same element
– They only differ in mass because they have different number of neutrons
Isotopes
• ____ – no. of proton in the nucleus of
an atom.
• No. of ____ = No. of Electron (atoms have the
same no. of proton and electron)
* ____. = total no. of proton and neutron
= no. of p + no. of n
= whole no. which is closest to the
atomic mass
Atomic number
Proton
Mass no.
Each Element Differs from the preceding element by
having one more positive charge in its nucleus The number of protons in the nucleus of an atom
determines its identity
Atomic number
____ An uncharged particle with a
mass slightly greater than
that of the proton
_____ discovered
neutron by correctly
interpreting an experiment
from the bombardment of
beryllium with high-energy
alpha particle
Neutrons
James chadwick
PROTONS
_____ observed
that a cathode-ray tube
generates a stream of
positively charged particles
____established that alpha
particles are positively
charged particles from his
scattering experiment
Eugen Goldstein
Ernest Rutherford
