___ are positively charged ions.
Cations
Mass Number=
Protons + Neutrons
The atom is made up of 3 subatomic particles called
Protons, neutrons, and electrons
Isotopes are atoms of the same element that have different
a. numbers of protons. b. number of neutrons. c. numbers of electrons.
What is B. different number of neutrons?
The percent abundance of all of the isotopes of an atom should add to _______.
100%
____ are negatively charged ions.
Anions
A changing proton number results in
a new element?
Which element is shown and what is it's charge?
Oxygen, neutral
Chlorine has a mass number 35. How many protons, neutrons, and electrons does it have?
What is 17 protons, 17 electrons, 18 neutrons?
What is the difference between K-39 and K-40
K-39 has 20 neutrons, K-40 has 21 neutrons
What is the charge of an atom with 24 protons, 24 neutrons, and 26 electrons?
What is -2?
What on the periodic table equals the number of protons in an atom's nucleus?
Atomic Number
Draw a carbon atom with a -4 charge.
I'll walk around and check
Write Calcium-40 in this isotope notation M AE?
What is 4020 Ca?
Draw a Sodium atom with a +3 charge.
Neutrons: 12
Electrons: 8
If a nitrogen atom has a charge of -3, how many electrons must it have?
10
In the isotope notation Silicon-28, the number 28 represents the
Atomic mass number
The space between the nucleus and the outer boundary of an atom is filled with mostly_______.
Empty space
If Bromine has three isotopes, Br-78, Br-80, Br-81, which would have the highest relative abundance?
Br-80
How many electrons can fit on the third energy level?
18
What will happen to an atoms charge as it loses electrons?
It will become more positive
Isotopes have the same number of ______ but different number of _________.
Protons, neutrons
Draw the isotope Boron-13.
Protons: 5
Electrons: 5
Neutrons: 8
Calculate the average atomic mass of boron given that 19.8% of its naturally occurring atoms have a mass of 10.013 amu and 80.2% have a mass of 11.009 amu.
10.812
Calculate the atomic mass of lead. The four lead isotopes have atomic masses and relative abundances of 203.973 amu (1.4%), 205.974 amu (24.1%), 206.976 amu (22.1%) and 207.977 amu (52.4%).
207.2 amu