chap 6 Flashcards
going down a group of the periodic table what patterns would you notice?
- atomic size increases
- ionic size increases
- ionization enegry decreases
- electronegativity decreases
- nuclear charge increases
- shielding increases
Going across a period what patterns would you notice?
- Atomic size decreases
- ionization energy increases
- electronegativity increases
- nuclear charge increases
- shielding is constant
elements were first classified according to what
their properties
who created the periodic table
Mendeleev
on mendeleevs periodic table how were elements placed
in increasing atomic mass
what did Mendeleev discover thru his table
the properties of unknown elenments
what is the modern day table organized by
atomic number
metals are…
good conductors and many are ductile and malleable
nonmetals are…
mostly gase whose properties are opposite to those of metals
metaloids can…
behave like metals or nonmetals depending on condition
How many elements had been identified by the year 1700?
13
What caused the rate of discovery to increase after 1700?
Chemists began to use scientific methods to search for elements
What did chemists use to sort elements into groups?
Chemists used the properties of elements.
Who was Dmitri Mendeleev?
he created a periodic table
What property did Mendeleev use to organize the elements into a periodic table?
arranged the elements in order of increasing atomic mas
what are 3 things u can name by looking at an element on the periodic table
- atomic number
- atomic mass
- what type of element it is
what is a valence electron
outer edge
Why are Group A elements called representative elements?
They exhibit a wide range of physical and chemical properties
Description of Electron Configuration for noble gases
s or p sublevels are filled
Description of Electron Configuration for Representative elements
s or p sublevels are only partially filled
Description of Electron Configuration for transition metals
s sublevel and nearby d sublevel contain electrons
Description of Electron Configuration for inner transition metals
s sublevel and nearby f sublevel contain electrons
letter of the elements found in the p block
Groups 3A, 4A, 5A, 6A, 7A, and 8A except helium
Ions form when…
atoms gain or lose electrons.
A positively charged cation forms
when an atom loses one or more electrons.
negatively charged anion forms
s when an atom gains one or more electrons.
First ionization energy
is the amount of energy required to remove one electron from
a neutral atom
Ionization energy tends to decrease from
top to bottom within a group
an
increase from left to right across a period.
A cation is
smaller than the atom that formed it
an anion
is larger than the atom that
formed it.
Ionic size generally increases
from top to bottom within a group
Ionic size generally decreases
from left to right across a period.
Electronegativity tends to decrease from
top to bottom
Electronegativity tends to increase from
from left to right across a period.
What is the general trend in atomic size within a group?
The atomic size increases within a group as atomic number increases. The atomic size
decreases from left to right across a period
What are the two variables that affect atomic size within a group?
- the charge on the nucleus
- the number of occupied energy levels
What is an ion?
an atom or group of atoms that has a positive or negative charge
How are ions formed
An ion is formed when electrons are transferred between atoms.
An ion with a positive charge is called a(n)
cation
an ion with a negative
charge is called a(n)
anion
anions
- neg
- nonmetal
- minus sign
cations
- pos
- metal
- plus sign
Why does ionization energy tend to decrease from top to bottom within a group?
Atomic size increases from top to bottom within a group. The nuclear charge
has a smaller effect on the electrons in the highest occupied energy level, so less
energy is required to remove an electron.
