Exam 1- Quantitative Chemistry

aluminum

what element is this?

Al

Iodine

what element is this?

I

Barium

what element is this?

Ba

Lithium

what element is this?

Li

Boron

what element is this?

B

Magnesium

what element is this?

Mg

Bromine

what element is this?

Br

Nickel

what element is this?

Ni

calcium

what element is this?

Ca

Nitorgen

what element is this?

N

Carbon

what element is this?

C

Oxygen

what element is this?

O

Chlorine

what element is this?

Cl

Phosphorus

what element is this?

P

Copper

what element is this?

Cu

Silicon

what element is this?

Si

Fluorine

what element is this?

F

Sulfur

what element is this?

S

Hydrogen

what element is this?

H

Zinc

what element is this?

Zn

Antimony

Stibium

What element is this, and what word does the symbol come from?

Sb

Gold

Aurum

What element is this, and what word does the symbol come from?

Au

Iron

Ferrum

What element is this, and what word does the symbol come from?

Fe

Lead

Plumbum

What element is this, and what word does the symbol come from?

Pb

Mercury

Hydragyrum

What element is this, and what word does the symbol come from?

Hg

Potassium

Kalium

What element is this, and what word does the symbol come from?

K

Silver

Argentum

What element is this, and what word does the symbol come from?

Ag

Sodium

Natrium

What element is this, and what word does the symbol come from?

Na

Tin

Stannum

What element is this, and what word does the symbol come from?

Sn

Tungsten

Wolfram

What element is this, and what word does the symbol come from?

W

hydrogen, oxygen, carbon, and nitrogen

what are the four most abundant elements in the human body?

the body cannot produce enough hemoglobin, so RBC’s can’t carry oxygen

what happens if there is not Iron (Fe) in the blood?

atomic number

number of protons within the atom’s nucleus

unique to each element

periods

horizontal rows

same ___ = same number of electron shells (energy levels)

groups (families)

vertical rows

same # of valence electrons + similar chemical behaviors

Alkali metals

What is Group 1 called?

Alkaline Earth Metals

What is Group 2 called?

Halogens

What is Group 7 called?

noble gases

What is ground 8 called?

main group elements

Consists of elements in groups 1,2, 13-18

Include some of the most common elements on earth

Properties tend to be more predictable & fall more reliably into patterns

transition elements (transition metals)

groups 3-12

Include most common metals used in everyday life (ie iron, nickel, copper, etc)

Important in nutrition & enzyme function

they are important for nutrition and enzyme function

Why are transition metals important to the body?

inner transition elements

Fit into the periodic table in periods 6 & 7 (after lanthanum [La] & actinium [Ac])

Belong to group 3 → placed under the table to make the width of the table more manageable

lanthanoids

what are elements 58-71 called?

actinoids

what are elements 90-103 called?

called rare earth elements

some are relatively common in Earths crust

what is another name for inner transition elements and what is the exception to this?

water aquifers

what is a common application of Cerium?

rechargeable batteries

camera lenses

what is a common application of lanthanum?

strong magnets

wind turbines

hybrid car motors

what is a common application of dysporium?

malleable

ability to be pounded into sheets

ductile

ability to be drawn into wire

metals

Majority of the elements located on the left side of the table

shiny luster

good electrical

good thermal conductivity

malleability

what are properties of metals?

nonmetals

Consists of most elements to the right + hydrogen

dull (not shiny) color

non-conductivity of heat & electricity

brittleness as solid

what are properties of nonmetals?

Boron (B)

Silicon (Si),

Germanium (Ge)

Arsenic (As)

Antimony (Sb)

Tellurium (Te),

Polonium (Po)

what are the 7 elements that are classified as metalloids on the “staircase”?

“Boring Silly Geese Ask Sbilly Teachers Politely”

• matter is made up of atoms that are indivisible

• each atom of an element has the same mass & is unique

• atoms combine to form compounds and combine in small, whole number ratios

• atoms of different elements can be combined to form new substances

what were the four parts of Dalton’s atomic theory?

• atoms are indivisible → they are actually divisible

• atoms have the same mass + unique to each element → atoms have isotopes and ions

what two parts of Dalton’s Atomic Theory were wrong?

proton and neutron

What two subatomic particles primarily compose the mass of an atom?

ions

Atoms that carry a positive of negative charge

Form when atoms gain or lose ELECTRONS

Isotopes

atoms of the same chemical element that have the same number of protons but different numbers of neutrons (ie different masses)

atomic mass unit (u)

standard unit for atomic‑scale masses.

6.02 x 10²³ u = 1 g

weighted average

type of average where each data point is multiplied by a "weight" or importance factor, then summed and divided by the total weights

often called the atomic mass

(weight x atomic mass) + …

how do you calculate atomic mass?

Electromagnetic spectrum:

the range of electromagnetic radiation from radio waves to gamma rays, characterized by wavelength & frequency (ie energy carried by light waves.)

short wavelength

high frequency

gamma rays have a ___ wavelength and a ___ frequency

long wavelengths

low frequency

radio rays have a ___ wavelength and a ___ frequency

Wavelength

the distance between two peaks of a wave

Frequency

number of waves that travel past a given point per second

long

low

___ wavelength → low frequency → ____ energy

Atomic spectrum

A unique pattern of absorbance & emission of electromagnetic radiation by an element.

electrons move to higher energy levels.

What happens to gaseous atoms when they are energized?

Each wavelength corresponds to a specific amount of energy released when electrons fall back to lower energy levels.

Why do atomic spectra show specific wavelengths?

Electrons can only exist in discrete (fixed) energy levels, not in between.

What does it mean that electrons occupy quantized energy levels?

Flame colors occur when electrons move between energy levels and emit light.

What causes flame test colors?

They are used to identify elements, especially metals.

What are atomic spectra and flame tests used for?

Principal energy levels, n

group of orbitals w/ similar energy.

Energy levels move farther from the nucleus and increase in energy.

How do energy levels change as n increases?

They have low energy and occupy a small three-dimensional space.

What are the characteristics of electrons in n = 1?

2 electrons

How many electrons can energy level n = 1 hold?

8 electrons; sublevels 2s and 2p.

How many electrons can energy level n = 2 hold and what are its sublevels?

18 electrons; sublevels 3s, 3p, and 3d.,

How many electrons can energy level n = 3 hold and what are its sublevels?

32 electrons; sublevels 4s, 4p, 4d, and 4f.

How many electrons can energy level n = 4 hold and what are its sublevels?

contain s, p, d, and f sublevels

What sublevels exist in energy levels n = 5–7?

A region in an atom where an electron is likely to be found.

orbital

A maximum of 2 electrons.

How many electrons can one orbital hold?

1 orbital and 2 electrons.

How many orbitals and electrons are in an s sublevel?

3 orbitals and 6 electrons.

How many orbitals and electrons are in a p sublevel?

5 orbitals and 10 electrons.

How many orbitals and electrons are in a d sublevel?

7 orbitals and 14 electrons.

How many orbitals and electrons are in an f sublevel?

Spherical with no directional orientation.

What is the shape of s orbitals?

Orbital size increases as energy level increases (1s < 2s < 3s).

How does the size of s orbitals change?

Two-lobed, figure-eight shape.

What is the shape of p orbitals?

pₓ along x-axis, pᵧ along y-axis, p_z along z-axis.

What are the orientations of p orbitals?

Complex, often clover-like; 5 orbitals.

What is the shape and number of d orbitals?

Very complex, multi-lobed; 7 orbitals.

What is the shape and number of f orbitals?

Greater complexity reflects more possible electron arrangements.,

Why do orbital shapes become more complex from s to f?

Radioactive decay

A process in which an unstable nucleus of an atom releases energy by ejecting a particle from the nucleus or by capturing an electron from the atom’s inner shells.

radioactive

The property of an unstable atom that makes it eject particles from the nucleus.

Nuclear radiation

The energy and particles that are given off by radioactive isotopes.