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Chemistry 11 > Unit 2 Chapter 1 > Flashcards

Unit 2 Chapter 1 Flashcards

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1
Q

octet rule

A

tendency to prefer to have 8 electrons in the valence shell

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2
Q

empirical knowledge

A

obtained through results of experiments

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3
Q

theoretical knowledge

A

obtained through observations

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4
Q

*An attempt to use familiar ideas
to describe unfamiliar things in a
visual way.
*It can be changed as new
information is collected.

A

scientific model

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5
Q

Democritus VS Aristotle

A

Things are made of atoms VS 4 earth elements

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6
Q

Dalton’s Billiard Ball Model

A

THOUGHT atoms were indivisible (False)
Atoms of the same element have identical properties. ✅

  1. Atoms of different elements combine
    in constant ratios to form compounds
    (Law of Constant composition)✅
  2. Chemical reactions involve the
    rearrangement of atoms; no new
    atoms are created or destroyed (Law
    of Conservation of Mass) ✅
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7
Q

Thomson

A

Empirical Evidence:
*As an electric current passed through a
gas, it gave off rays of negatively
charged particles.
* However, the gas was surprisingly
uncharged (neutral).
Conclusions:
*A particle smaller than an atom had to
exist.
– negative charges (e-s) came from
within the atom

ATOM WAS DIVISIBLE!

THOUGHT *There must be positively charged
particles in the atom, but he could never
find them.

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8
Q

Plum pudding

A

Thomson

FOUND ELECTRONS !!!

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9
Q

involved firing a stream
of tiny positively
charged alpha particles
at a thin sheet of gold
foil
* expected positive
charges to be spread
out evenly and
not enough to stop an
alpha particle

A

Rutherford’s Gold foil experiment

Empirical Evidence:
*Most of the positively charged alpha particles passed
straight through the gold foil.
*Some of the positively charged alpha particles
bounce away from the gold foil as if they
had hit something solid.

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10
Q

Rutherford’s Gold Foil Experiment Conclusion

A

Conclusions:
*Gold atoms in the sheet were mostly empty space.
– Atoms were not a pudding filled with a positively
charged material (Thompson).

*An atom has a small, dense, positively charged
center (i.e. NUCLEUS) that repelled the
positively charged alpha particles.

.: Nucleus is tiny compared to the atom as a whole.

HE FOUND PROTONS

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11
Q

_______ Model by rutherford

A

all of an atom’s positively charged
particles were
contained in the
nucleus.
* Negatively charged
particles were
scattered outside the
nucleus around the
atom’s edge.

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12
Q

Student of Rutherford - Chadwick

A

modified
Rutherford’s Mostly
Empty Space model
* atoms have a third
subatomic particle
being

NEUTRONS
in the nucleus

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13
Q

Bohr’s Planetary Atom Model

A

Electrons orbit the nucleus in circular
paths of fixed energy (ENERGY LEVELS).
* Electrons can jump (i.e.
transition) from energy level
to energy level.
* The higher the energy level, the
further it is away from the nucleus.
* PHOTONS are bundles of light
energy that that are emitted by
electrons as they go from higher
energy levels to lower energy levels.

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14
Q

ground state + excited state

A

Ground state is the lowest possible
energy level an
electron can be at.

excited state is an energy level
higher than the
ground state.

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15
Q

P.E.N

A

subatomic particles

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16
Q

Atoms of the same
element that have
a different #s of neutrons
yet they look, act
and react the
same.

A

isotopes

17
Q

device to identify isotopes

A

mass spectrometer

18
Q

Dobereiner

A

noticed a similarity
among the physical &
chemical properties
within several groups of
3 elements

  • LAW OF TRIADS
    – middle element had a
    mass about halfway
    between the atomic
    masses of the other two
19
Q

Newlands

A

arranged all known
elements in order of
increasing atomic
mass

  • LAW OF OCTAVES
    – repeating physical
    and chemical
    properties every 8
    elements
20
Q

Mendeleev

A

grouped elements with
similar properties in the
same column
– left blank spaces to add
elements

  • PERIODIC LAW
    – elements arranged by
    increasing atomic mass
    show a periodic
    recurrence of properties
    at regular intervals
21
Q

Modern periodic law

A

When the internal
structure of atoms was
discovered,
Mendeleev’s Periodic
Law was revised
– elements arranged by
increasing atomic #
show a periodic
recurrence of properties
at regular intervals

22
Q

sits atop group 1, but
it is not a member of
that family
* class of its own
* gas at room
temperature
* 1 p+ and 1 e-

in its
only energy level
* only 2 e-

to fill up its

valence shell

A

hydrogen

23
Q

group 1
* 1 valence e-
* most reactive
metals
– with halogens and
oxygen
– violently with water
to make a base
* soft, silver, solids
@ SATP

A

alkali metals family

24
Q

alkaline earth metals family

A

group 2
* 2 valence e-s
* react slowly with
water
* solid @ SATP
* react with air to form
oxides
* react with H+ to form
hydrides (except Be)

25
Q

groups 3 – 12
* strong, hard metals,
high melting points
* good conductors
* some form
multivalent ions
* variable reactivity
– many react with
oxygen to make
oxides
– some react with
acids

A

transition metals

26
Q

7 metalloids along the staircase divides
metals on left from non-metal on right.

A

B, Si, Ge, As, Sb, Te, Po

27
Q

halogens

A

group 17 non-metals
* 7 valence e-s
* extremely reactive
with hydrogen and
metals
* solid, liquid or gas
* dull, do not conduct
electricity

28
Q

noble gases

A

group 18 non-
metals

  • full valence shell
  • extremely un-
    reactive (stable)
  • low melting &
    boiling points
29
Q

atomic # 57 - 70
* rare earth
metals
* belong to the 6th
period

A

lanthanides

30
Q

Actinides

A

atomic # 89 – 102
* belong to the 7th period
* include elements
which are radioactive
and synthetic
* atomic #93+
(transuranic
elements) are
synthetic

31
Q

w/in a period, chemical reactivity is high in group 1,
lower towards the middle of P.T., maximum in group
17, and lowest in group 18.
* w/in a group, the chemical reactivity of metals
increase moving down while non-metals decrease
moving down.

A
32
Q

Lewis Diagrams

A

Lewis diagrams represent valence
electrons involved in bonding
–A chemical symbol represents the
nucleus and core electrons (not
involved in bonding).
–Dots around the symbol represent
valence electrons.

33
Q
  1. Write the element symbol.
  2. Draw dots, one for each valence electron
  3. Dots should be spread over 4 sides
  • It does not matter what side the dots are placed, but
    do not start to pair dots until there is one on each side
A

The number of valence electrons is equal to the
group number (for groups 1-3, 14-18), with
one exception. Which element is it?
Helium has 2 valence electrons in group 18

34
Q

atomic radius

A
  • the distance from the nucleus to just beyond the outermost electrons (valence electrons). In a diatomic molecule (such as nitrogen, N 2 , or oxygen, 0 2 ), the atomic radius is defined as the distance between the two nuclei, divided by 2
35
Q

Every electron in an atom experiences a force of attraction toward the nucleus

A

effective nuclear charge

36
Q

This occurs because the electrons of the inner levels ___ the outer electrons from the full charge of the nucleus. As a result, the outer electrons are not as strongly attracted by the nucleus, resulting in a larger atomic radius.

A

electron shielding

37
Q

ionic radius

A

a measurement of the size of an ion, usually expressed in picometres (pm); the distance from the centre of an ion to the outermost electrons

38
Q

representative elements

A

group 1, 2, 13-18 pg 31

Chemistry 11 (7 decks)

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